Answers
The chemical equation will be written as:
2C2H6 + 7O2 → 6H2O + 4CO2
What is ac Chemical Equation?Chemical formulas and symbols are used in chemical equations to depict a chemical reaction symbolically. A plus sign is placed between each entity in the reactants and products, and an arrow pointing in the direction of the products indicates the direction in which the reaction is taking place. The reactant entities are listed on the left and the product entities on the right. Chemical equations can be interspersed with structural (pictorial diagrams), symbolic, or both types of formulations. The absolute values of the stoichiometric numbers are represented by the coefficients placed next to the symbols and formulas of the entities.An arrow symbol, a series of reactants (the chemicals used to initiate the chemical reaction), and a list of products (the substances created during the chemical reaction) make up a chemical equation. Each substance is described by its chemical formula, which is sometimes followed by a figure known as the stoichiometric coefficient.Therefore,
The chemical equation will be written as:
2C2H6 + 7O2 → 6H2O + 4CO2
The Law of Conservation of Mass provides the foundation for balancing chemical equations. Stoichiometric coefficients must be added to products and reactants in order to balance the chemical equations. This is essential because all chemical equations must adhere to the laws of constant proportions and mass conservation, which dictate that the product side and reactant side of the equation must have the same number of atoms of each element.To learn more about Chemical Equations, refer to:
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Related Questions
Drag each tile to the correct location.
What types of mixtures are these?
peanuts and almonds mixed
food coloring dissolved in water
cup of tea and sugar
together in a bowl
a bucket full of sand and gravel
Homogeneous Mixture
Heterogeneous Mixture
Answers
Hetergeneous mixture peanuts and almonds mixed ,a bucket full of sand and gravel. Homogeneous Mixture -food coloring dissolved in water together in a bowl,cup of tea and sugar .
A Heterogeneous Mixture: what is it?When the composition of a mixture is not constant throughout the mixture, the mixture is said to be heterogeneous. A variety of make up vegetable soup. Each mouthful of soup will have variable proportions of the soup's various veggies and other ingredients.
Describe homogenous mixture using an example.For illustration A mixture of sugar and water, or salt and water, both of which have the same component ratio throughout the mixture, are examples of homogenous mixes.
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The energy released when a nucleus forms is calledQuestion 26 options: enthalpy. atomic mass. a becquerel. binding energy.
Answers
The correct answer in this case is binding energy, which is the energy released when a collection of nucleons form a nucleus.
The correct answer is the last choice.
4. Collaborate with a partner, make a brochure that highlights an example of a
technology that you have seen in which density is important.
Answers
The common use of density in ships and submarines is to predict whether or not a thing will float. Objects that have densities lower than those of water will sink if their densities are lower than water's.
What does density mean ?A product's density is a measure of how heavy it is relation to its size. If added to water, an object will float if its density is less than that of the water, while it will sink if its higher density. The density of a material is a distinguishing quality that is independent of the substance's volume.
Why is density important in chemistry?Because density is an intense property, it remains constant regardless of how much of a substance is present. Because it enables us to predict which compounds will float and which will sink in a liquid, density is a crucial notion.
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30.Vegetable soup is classified as which of the following?Select one:a. An atom.b. A compound.c. An element.d. A mixture.
Answers
A mixture in Chemistry is defined as a material made up of two or more different chemical substances, and it will not present a homogeneous solution, but instead a heterogeneous appearance, just like a vegetable soup, which is a mixture of many substances, answer letter D
Tablet salt (sodium chloride) is an example of a(n): A) element B) compound C) mixture
Answers
Sodium chloride contains sodium and chlorine in its structure. Both are elemens, which means that sodium chloride is a compound.
It is not a mixture since it is not made of 2 different substance. It is a substance made of 2 elements, which means it is a compound.
The correct answer is B) compound.
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.950 kg of water decreased from 103 °C to 60.5 °C.
Property Value Units
Melting point 0 °C
Boiling point 100.0 °C
ΔHfus 6.01 kJ/mol
ΔHvap 40.67 kJ/mol
cp (s) 37.1 J/mol · °C
cp (l) 75.3 J/mol · °C
cp (g) 33.6 J/mol · °C
Answers
The energy change when the temperature of 0.950 kg of water decreased from 103 °C to 60.5 °C is 2308.87 kJ.
What is the heat energy change when the temperature of 0.950 kg of water decreased from 103 °C to 60.5 °C?The heat energy change when the temperature of 0.950 kg of water decreased from 103 °C to 60.5 °C is determined from the formulas below:
Heat change 1 = Heat capacity as gas * moles * temperature change
Heat change 2 = Heat of vaporization, ΔHvap * moles
Heat change 3 = Heat capacity as liquid, Cp (l) * moles * temperature change
moles of water = 950 kg * 1000 g/kg * 1 mol/ 18g = 52.78 mole
Heat change 1 = 33.6 * 52.78 * (103 - 100) = 5320.224 J
Heat change 2 = 40.67 * 1000 * 52.78 = 2146562.6 J
Heat change 3 = 75.3 * 52.78 * (100 - 60.5) = 156986.193 J
Total heat change = 5320.224 J + 2146562.6 J + 156986.193 J
Total heat change = 2308869.017 J = 2308.87 kJ
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Consider the reaction between sodium metal and chlorine gas to form sodium chloride (table salt):2 Na(s) + Cl2 (g) > 2 NaCI(s)If 12.5 g of sodium react with sufficient chlorine, how many grams of sodium chloride should form?1. 12.1 grams2. 1.18 x 10^2 grams3. 15.9 grams4. 3.18 x 10^1 grams5. 51.0 grams
Answers
Answer:
[tex]4\text{ : 3.18 }\times\text{ 10}^1\text{ grams}[/tex]Explanation:
Here, we want to calculate the mass of sodium chloride formed
Firstly, we need to get the number of moles of sodium that reacted
To get this, we divide the mass of sodium by its atomic mass
We have that as:
[tex]\frac{12.5}{23}\text{ = 0.5435 mole}[/tex]Now, let us get the number of moles of chlorine
From the equation of reaction, 1 mole of sodium produced 1 mole of sodium chloride
Thus, 0.5435 mole of sodium will also produce 0.5435 mole of sodium chloride
To get the mass of sodium chloride formed, we multiply the above number of moles by the molar mass of sodium chloride
The molar mass of sodium chloride is 58.44 g/mol
Thus, the mass of sodium chloride formed will be:
[tex]58.44\text{ }\times\text{ 0.5435 = 31.8 g}[/tex]A chemist determined by measuring that 0.0750 moles of calcium participated in a chemical reaction. Calculate the mass of the calcium that participated in the chemical reaction. Be sure your answer Has the correct number of significant digits.?g
Answers
The mass of 0.0750 moles of calcium is 3.01g.
To calculate the mass of calcium we need to use the molar mass that we can find in the Periodic Table of Elements.
The molar mass of calcium is 40.1 g/mol.
Now, with a mathematical Rule of Three we can calculate the mass of calcium of 0.0750 moles:
[tex]\begin{gathered} 1\text{ mol Ca \_\_\_\_\_\_\_\_ 40.1 g} \\ \text{ 0.0750 mol \_\_\_\_\_\_\_ x = }\frac{0.0750\text{mol . 40.1g }}{1\text{mol}} \\ \\ x=3^{}.01\text{ g} \end{gathered}[/tex]So, the mass of 0.0750 moles of calcium is 3.01g.
The value of AH rxn for the following reaction is -72 kJ. How many kJ of heat is released when 0.989 g of HBr (80.91 g/mol) is formed? H2 (g) + Br2 (g) -› 2 HBr (gram). A. -144B. -72 C. -0.44 D. -36
Answers
Answer:
[tex]C\text{ : -0.44 KJ}[/tex]Explanation:
Here, we want to get the amount of heat released in KJ
From the change in enthalpy given and the equation of reaction, we know that 2 moles of HBr would lead to that amount of heat
Now, let us get the actual amount of heat released
We need to get the actual number of moles of HBr produced
Mathematically, we can calculate that by dividing the mass of HBr by its molar mass
We have that as:
[tex]\frac{0.989}{80.91}\text{ = 0.0122 mol}[/tex]From the reaction information:
-72 KJ was released by 2 moles
x KJ would be released by 0.0122 mol
To get the value of x, we have it that:
[tex]\begin{gathered} x\text{ }\times2\text{ = 0.0122 }\times\text{ \lparen-72\rparen} \\ \\ x\text{ = -36 }\times\text{ \lparen0.0122\rparen = -0.44 KJ} \end{gathered}[/tex]How many liters of oxygen gas at STP are required to react with 30.25 g of aluminum in the production of aluminum oxide?
Answers
Answer:
18.82L of oxygen gas are needed.
Explanation:
1st) It is necessary to write and balance the chemical reaction:
[tex]3O_2+4Al\rightarrow2Al_2O_3[/tex]2nd) From the balanced reaction, we can see that 3 moles of oxygen gas (O2) react with 4 moles of aluminum (Al). To convert moles to grams, it is necessary to use the molar mass of oxygen (32g/mol) and aluminum (27g/mol):
- O2 conversion:
[tex]\begin{gathered} 1mol-32g \\ 3mol-x=\frac{3mol*32g}{1mol} \\ x=96g \end{gathered}[/tex]- Al conversion:
[tex]\begin{gathered} 1mol-27g \\ 4mol-x=\frac{4mol*27g}{1mol} \\ x=108g \end{gathered}[/tex]Now we can see that 96g of O2 react with 108g of Al.
3rd) We have to calculate the grams of O2 that will react with 30.25g of Al:
[tex]\begin{gathered} 108gAl-96gO_2 \\ 30.25gAl-x=\frac{30.25gAl*96gO_2}{108gAl} \\ x=26.89gO_2 \end{gathered}[/tex]Using the molar mass of oxygen, we know that 26.89g represent 0.84 moles of O2.
4th) Finally, a mole of a gas at STP conditions occupies a volume of 22.4L. With this number and the moles of oxygen gas, we can calculate the liters:
[tex]\begin{gathered} 1mol-22.4L \\ 0.84mol-x=\frac{0.84mol*22.4L}{1mol} \\ x=18.82L \end{gathered}[/tex]So, 18.82L of oxygen gas are needed.
PART 1Select Introduction, and for the following unbalanced reactions found in the sim provide the missing coefficients.CoefficientReactant1CoefficientReactant2CoefficientProduct1CoefficientProduct2N2+H2HONH3H2O2COz
Answers
They give us the reactions with their respective products and reactants. To balance a reaction we must bear in mind that matter is neither created nor destroyed, it only transforms. So the mass that we have in the reactants must be the same in the products. We verify this by counting the atoms of each element on each side of the reaction.
In the first reaction we have nitrogen and hydrogen. We have 2 nitrogens and 2 hydrogens in the reactants. We start off-balanced in nitrogen, so we place coefficient 2 in the NH3 molecule to get 2NH3. Now that we have 2 nitrogens and 6 hydrogens in the products, we must balance the hydrogen in the reactants. For that, we place the coefficient 3 in the H2 in such a way that there will be 6 hydrogen atoms in the reactants. The equation is balanced and will be:
[tex]N_2+3H_2\rightarrow2NH_3[/tex]We do this same procedure for the other two equations. We count the atoms, we put the coefficients so that the number of atoms is conserved and we count again until the number of atoms of each element is the same on each side of the reaction. For the other two reactions we have:
[tex]2H_2O\rightarrow2H_2+O_2[/tex][tex]CH_4+2O_2\rightarrow CO_2+2H_2O[/tex]12: from the following list, decide whether the following are Arrhenius bases or acids.•HCl•NaOh•HBr•H2SO4•NH4OH•H3PO4•HNO3•LiOH•Ba(OH)2•CsOH•HF•KOH
Answers
Answer:
The Arrhenius acids in the list are:
HCl, HBr , H2SO4 , H3PO4 , HNO3 , HF
The Arrhenius bases are:
NaOH , NH4OH , LiOH , Ba(OH)2 , CsOH and KOH
Explanation:
An Arrhenius acid increases the concentration of H+ ions while an Arrhenius acid increases the concentration of OH- ions
Thus, an Arrhenius acid would yield H+ ions on ionization while an Arrhenius base will yield OH- ions on ionization
The Arrhenius acids in the list are:
HCl, HBr , H2SO4 , H3PO4 , HNO3 , HF
The Arrhenius bases are:
NaOH , NH4OH , LiOH , Ba(OH)2 , CsOH and KOH
The reaction represented by the following equation is a reversible process. N2O4(g)➡️⬅️2NO2(g)If you were to allow 1 mol of NO2 to react in a sealed container for some time, what would you expect to find in the container?NO2 onlyN2O4 onlyNothing, the vessel would be emptySome N2O4 and some NO2
Answers
Explanation:
The reaction:
N2O4(g) <=> 2NO2(g)
Inicially 0 [1 mol/Volume]
Reacts +x -2x
Equilibrium +x [1 mol/Volume]-2x
[1 mol/Volume] means molarity
In a chemical reaction, chemical equilibrium is the state in which the forward reaction rate and the reverse reaction rate are equal. The result of this equilibrium is that the concentrations of the reactants and the products do not change.
Therefore, the answer: Some N2O4 and some NO2
A -13.68 gram of sample of iron is heated in the presence of excess fluorine. A metal Fluoride is formed with a mass of 27.64g. Determine the empirical formula of the metal fluoride.
Answers
Explanation:
A 13.68 g sample of iron is reacted in presence of excess fluorine and an iron fluoride with a mass of 27.64 g is formed.
We have to find the empirical formula of our compound. This compound has two elements: Fe and F. We can express it like:
metal fluoride = FeₐFₓ
Where a is the subscript of Fe and x is the subscript for F.
First we have to find the mass of F present in the compound. We know that our compound has a total mass of 27.64 g and the mass of Fe present is 13.68 g. Since it only has two elements we can find the mass of F.
mass of sample = mass of Fe + mass of F
mass of F = mass of sample - mass of Fe
mass of F = 27.64 g - 13.68 g
mass of F = 13.96 g
So we found that our sample has 13.96 g of F and 13.68 g of Fe. Now we can determine the number of moles of each element that are present in the sample by using their molar masses.
molar mass of Fe = 55.85 g/mol
molar mass of F = 19.00 g/mol
moles of Fe = 13.68 g * 1 mol/(55.85 g)
moles of Fe = 0.245 moles
moles of F = 13.96 g * 1 mol/(19 g/mol)
moles of F = 0.735 moles
By definition the empirical formula is "simplest whole number ratio of atoms present in a compound". So if we want to find the ratio between them we have to divide both of them by the smallest number.
a = subscript of Fe = 0.245/0.245 = 1
x = subscript of F = 0.735/0.245 = 3
So the empirical formula of our compound is:
empirical formula = FeₐFₓ
empirical formula = FeF₃
Answer: empirical formula = FeF₃
What is the theoretical yield when 1.1134 g of gold (III) oxide is reacted with 20.0 L of H2 at 1.000 atm and 800K.
Answers
The theoretical yield of the gold is 0985 g
What is the theoretical yield?Recall that the yield is defined as the mass of the product that is obtained in the reaction. Let us recall that a chemical reaction must involve the interaction of the reactants so as to obtain in a given amount, the products of the particular reaction that is in question.
Now;
Number of moles of the gold (III) oxide = 1.1134 g/442 g/mol = 2.5 * 10^-3 moles
We can get the number of moles of the hydrogen from the ideal gas equation;
PV = nRT
n = PV/RT
n = 1.000 atm * 20.0 L/0.082 atm LK-1mol-1 * 800K
n = 0.3 moles
Given that the mole ratio of the reaction is 1 mole of the oxide to three moles of hydrogen;
1 mole of gold (III) oxide reacts with 3 moles of hydrogen
2.5 * 10^-3 moles of gold (III) oxide reacts with 2.5 * 10^-3 moles * 3 moles /1 mole
= 7.5 * 10^-3 mole of hydrogen
Hence the hydrogen is present in excess.
The theoretical yield =
1 mole of the oxide produced 2 moles of the gold
2.5 * 10^-3 moles of the oxide produced 2.5 * 10^-3 moles * 2 moles/1 mole
= 5 * 10^-3 moles of gold
Theoretical yield = 5 * 10^-3 moles of gold * 197 g/mol
= 0985 g
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Can someone help me to answer this?As you reflect on how to interpret a balanced chemical reaction.Ammonium nitrate is a common fertilizer, but under the wrong conditions it can be hazardous. In 2002, Philippines has banned imports of ammonium nitrate that used in bombs that killed 12 people in Mindanao area.The explosion resulted from this reaction:2NH4NO3(s)→2N2(g)+4H2O(g)+O2(g)Construct a table showing how to interpret the information in the equation in terms of:1. individual molecules and ions.2. moles of reactants and products.3. grams of reactants and products given 2 mol of ammonium nitrate.4. numbers of molecules or formula units of reactants and products given 2 mol of ammonium nitrate.
Answers
(1)
The molecule NH4NO3 is ammonium nitrate, which makes a redox reaction.
It produces N2, O2, and H2O, which are nitrogen, oxygen, and water.
The ions are 2NH4+ and 2NO3-.
2 molecules of N2, 4 molecules of H2O, and 1 molecule of O2.
(2)
There are 2 moles of NH4NO3, 2 moles of N2, 4 moles of H2O, and 1 mole of O2.
(3)
The molar mass of NH4NO3 is 80.043 grams per mole, but there are 2 moles of it, so there are 160.09 grams of NH4NO3.
There are 56.03 grams of N2 because there are 2 moles of it. (1 mole N2 = 28.0134 g/mol).
There are 72.06 grams of H2O because there are 4 moles of it (1 mole H2O = 18.02 g/mol).
There are 31.998 grams of O2 because there's just 1 mole of it.
(4)
The formula units of NH4NO3 is 1.204x10^24, which is equivalent to 2 moles.
Nitrogen has the same formula units because there are 2 moles of it, so it's 1.204x10^24.
Water has 2.409x10^24 because there are moles of it.
Oxygen has 6.022x10^23 because there's just 1 mole, inis Avogadro's Number.
Define hydrogen bonding and explain how hydrogen are bonding involved in the
transfer of genetic material.
Answers
Answer:
Hydrogen bonding is a special type of dipole-dipole attraction between molecules, not a covalent bond to a hydrogen atom. It results from the attractive force between a hydrogen atom covalently bonded to a very electronegative atom such as a N, O, or F atom and another very electronegative atom.
Explanation:
Balance the following equation:ZnO(s)⟶ΔZn(l)+O2(g) Express your answer as a chemical equation. Identify all of the phases in your answer.
Answers
Answer:2ZnO(s)→2Zn(l)+O2(g)
Explanation:
7. A given sample of gas is held in a container with the volume of 6.02 L with a temperature of 59.5℃ at a pressure of 1.20 atm. What is the final pressure when the sample of gas is administered to a new volume of 10.0 L at 20.2℃?
Answers
The final pressure when the sample of gas is administered to the new volume and temperature is 0.64 atm.
What is the final pressure when the sample of gas?Combined gas law put together both Boyle's Law, Charles's Law, and Gay-Lussac's Law. It states that "the ratio of the product of volume and pressure and the absolute temperature of a gas is equal to a constant.
It is expressed as;
P₁V₁/T₁ = P₂V₂/T₂
Given the data in the question;
Initial volume V₁ = 6.02LInitial pressure P₁ = 1.20 atmInitial temperature T₁ = 59.5℃ = ( 59.5 + 273.15 )K = 332.65KFinal volume V₂ = 10.0L Final temperature T₂ = 20.2℃ = ( 20.2 + 273.15 )K = 293.35KFinal pressure P₂ = ?To determine the final pressure of the gas, plug the given values into the formula above and solve for P₂.
P₁V₁/T₁ = P₂V₂/T₂
P₁V₁T₂ = P₂V₂T₁
P₂ = P₁V₁T₂ / V₂T₁
P₂ = ( 1.20 atm × 6.02L × 293.35K ) / ( 10.0L × 332.65K )
P₂ = ( 2119.1604 KLatm ) / ( 3326.5 KL )
P₂ = 0.64 atm
Therefore, the final pressure of the gas is 0.64 atm.
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How many moles of H2 is needed to produce 12 moles of NH3
Answers
The balanced reaction is:
[tex]N_2+3H_2\rightarrow2NH_3[/tex]According to this, 3 moles of H2 produce 2 moles of NH3. Use this ratio to find the number of moles of NH3 produced:
[tex]12molNH_3\cdot\frac{3molH_2}{2molNH_3}=18molH_2[/tex]It means that 18 moles of H2 are needed to produce 12 moles of NH3
A student wants to produce a 1.8 M solution and has 0.9 moles of solute available. What is the maximum volume (in mL) of solution that can be produced?Given:Find:Equation used:Answer:
Answers
Answer:
[tex]500\text{ mL}[/tex]Explanation:
Here, we want to get the maximum volume of solution that can be produced
Given:
Molarity = 1.8 M
Number of Moles = 0.9 moles
Find:
Volume
Equation Used:
Number of moles = molarity * volume
Answer:
[tex]\begin{gathered} 0.9\text{ = 1.8 }\times\text{ V} \\ V\text{ = }\frac{0.9}{1.8} \\ V=0.5dm^3 \end{gathered}[/tex]To convert this to mL, we multiply the volume by 1000 since 1 L = 1000 mL
Thus, we have it that:
[tex]0.5\text{ }\times1000\text{ = 500 mL}[/tex]A sample of glass that has a mass of 9.3 g gives off 87 J of heat. If the temperature of the sample changes by 12.7°C during this change, what is the specific heat of the glass? NEED ASAP
Answers
Answer
The specific heat of the glass = 0.7366 J/g°C
Explanation
Given:
Mass of the glass sample, m = 9.3 g
Quantity of heat given off, Q = 87 J
Change in temperature, ΔT = 12.7 °C
What to find:
The specific heat, c of the glass.
Step-by-step solution:
The specific heat, c of the glass can be calculated using the given formula below.
[tex]\begin{gathered} Q=mc\Delta T \\ \\ \Rightarrow c=\frac{Q}{m\Delta T} \end{gathered}[/tex]Putting the values of the given parameters into the formula, we have;
[tex]c=\frac{87J}{9.3g\times12.7°C}=\frac{87\text{ }J}{118.11\text{ }g°C}=0.7366\text{ }J\text{/}g°C[/tex]Therefore, the specific heat of the glass is 0.7366 J/g°C
How many atoms of oxygen are in the reactants of the following equation? 3NO2 + H2O --> NO + 2HNO3
Answers
The reactants are the compounds before the arrow and the products are after the arrow. Just as they show us, the oxygen atoms in the reagents will bJust as the reaction shows, the oxygen atoms in the reactants will be:
Answer: There are 7 atoms of oxygen in the reactants
Which of the listed species have the following electron configuration?
(See attached)
Answers
Answer:
Al 3+
Na+
Mg2+
F-
Explanation:
The element with the given electron that isn't an ion is Neon. It has 10 electrons in total.
Looking at the periodic table attached will help to see how the elements below are related to the one circled in red (Ne).
Al 3+ lacks 3 (because it has a 3+ charge) of its normal electrons so it has 10 and will have the same electron configuration as shown.
Na+ lacks one electron so it will also have 10 electrons instead of its normal 11.
Mg 2+ lacks two electrons so it will also have 10 total electrons.
F- has gained an extra electron so it now has 10 instead of 9.
Al3+, Na+, F-, and Mg2+ will have the given electronic configuration.
The electronic configuration given in the question is:
2p6, 2s2, 1s2
If it was a stable atom, the answer would have been Neon.
And if that would have been negative ion or anion (to be precise),
the answer would have been either F- or O2-.
But in the case of positive ions or we can say cations,
Al3+, Na+, and Mg2+ have the given electronic configurations.
Because the atom of Aluminum loses three electrons to achieve another state which is responsible for the formation of Al3+.
Similarly,
The atoms of Sodium and Magnesium also lose one and two electrons respectively to form Na+ and Mg2+.
So, we can conclude that Al3+, Na+, F- and Mg2+ will have the given electronic configuration.
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Methane(CH4) gas and oxygen (O2) gas react to form carbon dioxide (CO2) gas and water vapor(H2O). Suppose you have 5.0 mol of CH4 and 1.0 mol of O2 in a reactor.
What would be the limiting reactant? Enter its chemical formula below
Answers
The limiting reactant, given that 5.0 moles of CH₄ and 1.0 mole of O₂ are in the reactor is O₂
How do I determine the limiting reactantWe'll begin by obtainig the balanced equation for the reaction. This is given below:
CH₄ + 2O₂ —> CO₂ + 2H₂O
The limiting reactant for the reaciont can be obtained as illustrated below:
From the balanced equation above,
1 mole of CH₄ reacted with 2 moles of O₂
Therefore,
5 moles of CH₄ will react with = 5 × 2 = 10 moles of O₂
From the above illustration, we can see that a higher amount of O₂ is needed to react completely with 5 moles of CH₄.
Thus, we can conclude that O₂ is the limiting reactant.
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SYNTHESIS OFCARBONATECTIONLABORATORY SIMULATIONLab Data- X99.00.10CollectedVolume sodium carbonate (mL)Molarity sodium carbonate (M)Volume calcium chloride (mL)Molarity calcium chloride (M)ObservationsThe mixture has now turned white100.00.20hemDisp0.211.30Mass filter paper (9)Mass filter paper + precipitate (9)CalculatedObserved mass calcium carbonate (9)Identify limiting reactantExpected mass calcium carbonate (9)Percent yield (%)0.88Calcium chlorideHow to calculate theoretical yield and percent yield
Answers
Answer:
[tex]\begin{gathered} \text{Limiting Reagent = Sodium Carbonate} \\ \text{Percent Yield = 98\%} \end{gathered}[/tex]Explanation:
The chemical reaction talks about the synthesis of calcium carbonate
It is from the reaction between sodium carbonate and calcium chloride
Let us write the equation of reaction as follows:
[tex]Na_2CO_{3(aq)}+CaCl_{2(aq)}\text{ }\rightarrow2NaCl_{(s)\text{ }}+CaCO_{3(aq)}[/tex]Firstly, we want to get the expected mass of calcium carbonate
This speaks about getting the theoretical yield based on the equation of reaction
From the data collected, 90 ml of 0.20 M (mol/L) of sodium carbonate gave calcium carbonate
We need to get the actual number of moles of sodium carbonate that reacted
We can get this by multiplying the volume by the molarity (kindly note that we have to convert the volume to Liters by dividing by 1000)
Thus, we have it as:
[tex]\frac{90}{1000}\times\text{ 0.1 = 0.009 moles}[/tex]Hence, we see that 0.009 moles of sodium carbonate reacted theoretically
Since 1 mole of sodium carbonate gave 1 mole calcium carbonate, it is expected that 0.009 mole of sodium carbonate will give 0.009mole of calcium carbonate
What we have to do now is to get the theoretical grams of calcium carbonate produced
That would be the product of the number of moles of calcium carbonate and its molar mass
The molar mass of calcium carbonate is 100 g/mol
The theoretical yield (expected mass) is thus:
[tex]100\text{ g/ mol }\times\text{ 0.009mol = 0.9 g}[/tex]Finally, we proceed to get the percentage yield which is calculated using the formula below:
[tex]\text{Percent Yield = }\frac{Actual\text{ yield}}{\text{Theoretical yield}}\times\text{ 100 \%}[/tex]The actual yield is the observed mass which is given as 0.88 g
The percent yield is thus:
[tex]\frac{0.88}{0.9}\times\text{ 100 = }98\text{ \%}[/tex]
What could be the third quantum number for one of the electrons in the 4penergy sublevel of bromine?A. m = -1B. m = 5C. m = +D. m = 4
Answers
Assuming the third quantum number is the question is the magnetic quantum number, it is limited by the angular momentum quantum number. This is inditaced in the quastion: since the orbital is 4p, the "p" indicates that the angular momentum quantum number is 1.
The magnetic quantum number can only be -1, 0 or +1.
The only alternative with one os these is alternative A.
A student has a sample of 1.31 moles of fluorine gas that is contained in a 24.6 L container at 336 K. What is the pressure of the sample? The ideal gas constant is 0.0821 L*atm/mol*K. Round your answer to the nearest 0.01 and include units.
Answers
Answer
The pressure of the sample is 1.47 atm
Explanation
Given:
Moles, n = 1.31 mol
Volume, V = 24.6 L
Temperature, T = 336 K
The ideal gas constant, R = 0.0821 L*atm/mol*K
What to find:
Pressure, P of the sample.
Step-by-step solution:
Pressure, P of the sample can be calculated using the ideal gas equation.
[tex]\begin{gathered} PV=nRT \\ \\ \Rightarrow P=\frac{nRT}{V} \end{gathered}[/tex]Put the values of the parameters into the formula, we have;
[tex]P=\frac{1.31mol\times0.0821\text{ }L.atm/mol.K\times336K}{24.6\text{ }L}=1.47\text{ }atm[/tex]The pressure of the sample is 1.47 atm
How many pounds in 16.1lbmol of pure HCl
Answers
Answer:
586.846 lbs
Explanation:
the molar mass of HCl is 1 + 35.45 = 36.45
this means you can do 16.1 lbmol * 36.45 lb/lbmol = 586.845
What is a molecular equation and what is this question asking please help?
Answers
In this question, we have a reaction between silver nitrate and potassium chloride, which will have the following chemical formula and also the following product:
AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq)
Now we need to identify the ions that are components of the precipitate that was formed in this reaction
A precipitate is a product of a reaction that is not soluble in water in the conditions given in the reaction, therefore the precipitate will be a solid product of the reaction. The solid of the reaction is AgCl, therefore this is the precipitate
Now the ions that compose AgCl are Ag+ and Cl-, the answer will be the 3rd option
