To solve this question we will use the integrated rate late law for first order reaction:
[tex]\begin{gathered} ln[A]=-kt+ln[A]_0 \\ [A]:concentration\text{ }of\text{ }A\text{ }at\text{ }certain\text{ }time=1.89mg \\ k:rate\text{ }constant=x \\ t:time=474\text{ }mins \\ [A]_0:initial\text{ }concentration=2.56mg \end{gathered}[/tex]By substituting the values we have to determine the unknown we get:
[tex]\begin{gathered} ln1.89=-k\times474min+ln2.56 \\ \frac{0.637-0.940}{-474min}=k \\ k=6.392\times10^{-4}\text{ }min^{-1} \end{gathered}[/tex]Answer: Rate constant k is 6.392x10^-4 per min.
The wavelength of green light from a traffic signal is approximately 5.2 * 10^7 m. Calculate its frequency
If the wavelength of green light from a traffic signal is approximately 5.2 ×10⁷ m , then the frequency of the light would be 5.769 × 10¹⁶ Hz .
What is Wavelength?It can be understood in terms of the distance between any two similar successive points across any wave for example wavelength can be calculated by measuring the distance between any two successive crests.
C = λν
The frequency of the green light = 3 × 10⁸ / 5.2 ×10⁷
= 5.769 × 10¹⁶ Hz
Thus , If the wavelength of green light from a traffic signal is approximately 5.2 ×10⁷ m , then the frequency of the light would be 5.769 × 10¹⁶ Hz .
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If I have 10.0g of Mg, what is my theoretical yield of MgCl2
Explanation:
First, let's write the balanced equation of formation of MgCl2 from Mg and Cl2:
Mg + Cl2 → MgCl2
Now let's transform 10.0g of Mg into moles, using the following formula: moles = mass/molar mass
molar mass of Mg = 24.3 g/mol
moles = 10/24.3
moles = 0.412 moles
Now we use the equation ratio between Mg and MgCl2 to find the quantity of MgCl2 in moles.
1 mole of Mg produces 1 mole of MgCl2.
So 0.412 moles of Mg produces 0.412 moles of MgCl2.
Now we transform 0.412 moles of MgCl2 into mass using the following formula: mass = moles x molar mass
Molar mass of MgCl2: 24.3 + (2*35.45) = 95.21 g/mol
Mass = 0.412 * 95.21
Mass = 39.2 g
Answer: The theoretical yield of MgCl2 is 39.2 g.
Light below the necessary critical frequency doesn't eject electrons from metal because
Light below the necessary critical frequency doesn't eject electrons from metal because no electrons will be emitted when the light shines on the metal.
What is Frequency?This is a term in physics which is used to describe the number of occurrences of a repeating event per unit of time.
The amount of energy which is present in each photon in the beam is determined by and proportional to the frequency of the beam. This therefore means that if there is light which is below the threshold frequency, there will be no electrons emitted when light shines on the metal thereby making it the correct choice.
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How many moles of chromium metal, Cr, are in a 260 gram piece of chromium?
In order to answer this question we will use the molar mass of Chromium, which is 52 g/mol, that means that in every 1 mol of Cr, we will have 52 grams of it:
52 g = 1 mol
260 g = x moles
52x = 260
x = 5 moles of Chromium
The volume of ammonia gas at .930 atm of pressure is gradually decreased from 96.2mL to 44.7mL. What is the final pressure of ammonia if there is no change in temperature?
Initial Pressure = P₁ = 0.930 atm
Final Pressure = P₂ = ?
Initial Volume = V₁= 96.2 mL
Final Volume = V₂ = 44.7 mL
Temperature = constant
If we consider that ammonia as an Ideal Gas, and since the temperature is constant we can apply Boyle's Law. It says that at constant temperature:
P₁ * V₁ = P₂ * V₂
If we divide at both sides by V₂:
P₁* V₁ / V₂ = P₂ * V₂ / V₂
On the right side we can cancel V₂ and we get:
P₁* V₁ / V₂ = P₂
P₂ = P₁* V₁ / V₂
Replacing by the values that we were given:
P2 = 0.930 atm * 96.2 mL / (44.7 mL)
P2 = 2.00 atm
So the final pressure is 2.00 atm
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.
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
Terrance found a small hair on the victim’s shirt. What type of evidence does this BEST represent?
A.
trace evidence
B.
biological evidence
C.
ammunitions evidence
D.
impression evidence
Answer:
Biological evidence, since it was a hair, which forms part of the human
Some hydrogen and iodine are mixed at 229 degrees Celsius in a 1.00L container. When equilibrium is established, the following concentrations are present: [HI] = 0.490 M, [H2] = 0.080 M, [I2] = 0.060 M. If an additional 0.300 mol of HI is then added, what concentration will be present when the new equilibrium is established?
The concertation of the HI that would be present in the new equilibrium position is 0.15 M.
What is the new equilibrium position?We have to first obtain the equilibrium constant that we have under the initial conditions and then we have; H2 + I2 ------> 2HI
K = [HI]^2/[H2] [I2]
K = (0.490)^2/(0.080) (0.060)
K = 0.2401/(0.080) (0.060)
K = 50
Again;
H2 + I2 ------> 2HI
Initial 0.080 0.060 0.060
concentration +x +x -2x
Equilibrium 0.080 + x 0.060 + x 0.490 - 2x
50 = (0.490 - 2x)^2/( 0.080 + x) (0.060 + x)
Working through the quadratic we have;
46x^2 + 10.2 x - 0.38 = 0
x = 0.32 M
In each case we now have;
H2 = 0.080 + 0.32 = 0.4 M
[I2] = 0.060 + 0.32 = 0.38 M
[HI] = 0.790 - 2( 0.32 ) = 0.15 M
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Fe2O3 + 3H2 = 2Fe + 3H2OCalculate how many grams of iron can be made from 24.5 grams of iron (III) oxide.
Explanation:
Iron (III) oxide will react with hydrogen gas to produce iron and water. They will react according to the following equation.
Fe₂O₃ + 3 H₂ -----> 2 Fe + 3 H₂O
We have to find the grams of Fe that can be made from 24.5 g of Fe₂O₃. So, first we have to convert those grams into moles using the molar mass of iron (III) oxide.
molar mass of Fe₂O₃ = 159.69 g/mol
mass of Fe₂O₃ = 24.5 g
moles of Fe₂O₃ = 24.5 g * 1 mol/(159.69 g)
moles of Fe₂O₃ = 0.153 mol
Fe₂O₃ + 3 H₂ -----> 2 Fe + 3 H₂O
According to the coefficients of the equation, we know that 1 mol of Fe₂O₃ will react with 3 moles of H₂ to give 2 moles of Fe and 3 moles of H₂O. So the molar ratio between Fe₂O₃ and Fe is 1 to 2. We can use that relationship to find the number of moles of Fe that can be made from 0.153 moles of Fe₂O₃.
1 mol of Fe₂O₃ : 2 moles of Fe molar ratio
moles of Fe = 0.153 moles of Fe₂O₃ * 2 moles of Fe/(1 mol of Fe₂O₃)
moles of Fe = 0.306 moles
So we found that we can produce 0.306 moles of Fe from 0.153 moles of Fe₂O₃ or 24.5 g of it. Finally we can convert the 0.306 moles of Fe into grams using the molar mass of Fe.
molar mass of Fe = 55.85 g/mol
mass of Fe = 0.306 moles * 55.85 g/mol
mass of Fe = 17.1 g
Answer: 17.1 g of iron can be made from 24.5 g of iron (III) oxide.
Determine the percent composition of hydrogen for the following: NaHCO3
By definition, the percent composition of an atom in a compound is its mass percentage in the formula.
That is, if we have 1 mol of NaHCO₃, we have also 1 mol of H (because there is only on H for each molecule).
So, we calculate the mass of this 1 mol of NaHCO₃ and the mass of 1 mol of H and calculate the percentage.
In equations, we want the following:
[tex]C_H=\frac{m_H}{m_{NaHCO_{3}}}[/tex]Since these are ratios, we doesn't matter if we talk about 1, 2 or any number of moles, but 1 mol is easier because the molecular and atomi masses are for 1 mol.
The molecular mass of NaHCO₃ is:
[tex]\begin{gathered} M_{NaHCO_3}=M_{Na}+M_H+M_C+3\cdot M_O \\ M_{NaHCO_3}\approx(22.990+1.008+12.011+3\cdot15.999)g/mol \\ M_{NaHCO_3}\approx84.006g/mol \end{gathered}[/tex]Which means that we have approximately 84.006 grams of NaHCO₃ in 1 mol of it.
The atomic mass of H is:
[tex]M_H\approx1.008g/mol[/tex]Which means that we have approximately 1.008 grams of H in 1 mol of it.
Now, we can take the percentage of mass of H:
[tex]C_H\approx\frac{1.008g_{}}{84.006g}\cdot100\%\approx1.20\%[/tex]So, the percentage composition of H in NaHCO₃ is approximately 1.20%.
Amanda is sending away hair samples to be tested for DNA. What is the BEST sample she can send to the lab for testing?
A.
hair from the telogen stage
B.
hair that has naturally shed
C.
hair with exposed follicular tissue
D.
hair that has been dyed
The sample of hair with exposed follicular tissue is the BEST sample she can send to the lab for DNA testing (Option C).
What is a DNA sample?A DNA sample is any tissue that can be used to extract DNA and therefore it is multipurpose because it can be used to identify an organism, identify polymorphisms, find gene variants associated with a phenotype of interest., etc.
Therefore, with this data, we can see that the sample of a follicular tissue contains DNA which can be used for different purposes such as the identification of an individual.
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Experiment 2: Copper(II) carbonate hydroxide produces one mole of water (=18.015 g/mol) for every two moles of solid product (=79.545 g/mol) produced. If 3.597 g of solid product were produced during the reaction, how many grams of water were realeased as water vapor?
C2H4 + 3O2 ——> 2CO2 + H2OWhat volume of oxygen at STP is needed to react with 5.75 mol of C2H4 (Show all work and data charts)
Explanation:
C₂H₄ + 3 O₂ ——> 2 CO₂ + H₂O
According to the coefficients of the equation 1 mol of C₂H₄ will react with 3 moles of O₂. Then, the molar ratio between C₂H₄ and O₂ is 1 to 3. We can use that relationship to find the number of moles of oxygen that are needed to react with 5.75 moles of C₂H₄.
1 mol of C₂H₄ = 3 moles of O₂
moles of O₂ = 5.75 moles of C₂H₄ * 3 moles of O₂/(1 mol of C₂H₄)
moles of O₂ = 17.25 moles
One mol of a gas at STP always occupies 22.4 L. We can use that relationship to find the volume of oxygen.
1 mol of O₂ = 22.4 L
volume = 17.25 moles of O₂ * 22.4 L/(1 mol of O₂)
volume = 386.4 L
Answer: 386.4 L at STP is needed to react.
When dealing with diatomic elements like oxygen, the atoms are not separate; they always come in pairs. Therefore, one mole of oxygen molecules would weigh _______ grams and not 16 grams
32 grams
Explanations:What are diatomic elements?Diatomic elements are elements that contain two atoms chemically bonded together.
When looking for the molar mass of a diatomic element, the number of atoms in the element is multiplied by the molar mass of the element.
For instance, oxygen is a diatomic element with the chemical symbol of O₂. This shows that the molar mass of oxygen will be given as:
[tex]\begin{gathered} molar\text{ mass of O}_₂=2\times16g\text{/mol} \\ molar\text{ mass of }O_2=32g\text{/}mol \end{gathered}[/tex]This shows that one mole of oxygen molecules would weigh 32 grams and not 16 grams.
If gas has a pressure of 536 and a volume of 645 liters and is 352 moles what is the new temp ?
To solve this question we have to use the ideal gas law:
[tex]PV=nRT[/tex]Where P is the pressure, V is the volume, n the number of moles, R the constant of ideal gases and T the temperature.
Solve the equation for T and replace for the given values. Remember that R has a value of 0.082atmL/molK:
[tex]\begin{gathered} T=\frac{PV}{nR} \\ T=\frac{536atm\cdot645L}{352mol\cdot\frac{0.082atmL}{molK}}=11977.54K \end{gathered}[/tex]According to this, the temperature of the gas is 11977.54K.
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Answer:
what is this free
branliest?
which of the following statements are consistent with dalton's atomic theory as it was originally stated?
a. Sulfur and oxygen atoms have the same mass.
b. All cobalt atoms are identical.
c. Potassium and chlorine atoms combine in a 1:1 ratio to form potass...
Option B. All cobalt atoms are identical and are consistent with dalton's atomic theory as it was originally stated.
The primary part of dalton's atomic theory states that everyone relies on is manufactured from atoms, which can be indivisible. the second part of the theory says all atoms of a given element are the same in mass and house. The 0.33 part says compounds are combos of two or more exceptional kinds of atoms.
Dalton's atomic theory, atoms of one element are all the equal or same. for this reason, the assertion that every cobalt atoms are identical is consistent with Dalton's concept of the shape of atoms.
Dalton's atomic concept additionally proposed that each atom of an element is identical in nature and exceptional elements vary in length, mass, and chemical properties. So, the accurate answer is choice 1 which says that the first and 2d statements are correct.
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Sn +Cl————SnCl4what is the limiting reactant when 15.7 g of tin reacts with 17.4 of chlorine? what mass of tin chloride can be formed?
Cl is the limiting reactant and the mass of tin chloride that can be formed is 31.9g.
- First, we need to balance the equation:
[tex]Sn\text{ + 4 Cl }\rightarrow SnCl_4[/tex]- Second, we need to know the molar weight of the compounds:
Sn: 118.7 g/mol
Cl: 35.5 g/mol
SnCl4: 260.7 g/mol
- Third, we need to know how much Sn can react with Cl according to the balanced equation:
[tex]\frac{15.7g\text{ . 142g}}{118.7g}=\text{ 18.8 g}[/tex]If 118.7g of Sn needs 142g of Cl to react according to the balanced equation, we found that the 15.7g of Sn will need 18.8g of Cl to complete the reaction.
As we have 17.4g of Cl available, we can see that we are going to need more Cl and therefore Cl is the limiting reactant.
- Now, to find the mass of tin chloride that can be formed, we use the limiting reactant amount for the calculation:
[tex]\frac{17.4g\text{ . 260.7g}}{142g}=31.9\text{ g}[/tex]According to the balanced equation we need 142g of Cl to produce 260.7g of tin chloride, so with 17.4g of chlorine we will obtain 260.7g of SnCl4.
So, the mass of tin chloride that can be formed is 31.9g.
Calculate the number of photons having a wavelength of 16.0 um required to produce 2.3KJ of energy (Note => 16.0 um = 16.0 * 10^6 m & 2.3KJ = 2300 J)
The number of photons having a wavelength of 16.0 um required to produce 2.3KJ of energy is 1.85 x 10¹⁹
What are photons?Photons are defined as a basic particle that is both the force carrier for the electromagnetic force and a quantum of the electromagnetic field, which includes electromagnetic radiation like light and radio waves.
It can also be defined as a discrete bundle of electromagnetic energy is what is known as a light particle.
Energy = 2.3 KJ
Wavelength = 16.0 x 10⁶ m
Energy = hc / ∧
= 6.63 x 10²⁴ x 3 x 10³ / 16.0 x 10⁶
= 1.24 x 10¹⁹ J
Number of photons used = 2.3 KJ / 1.24 x10¹⁹
= 1.85 x 10¹⁹
Thus, the number of photons having a wavelength of 16.0 um required to produce 2.3KJ of energy is 1.85 x 10¹⁹
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Which hydrogen below will have the greatest partial positive charge?Group of answer choicesHIHClHBrHFcannot determine
The hydrogen bonded to the most electronegative element will have the greatest partial positive charge. This is because electronegativity corresponds to the ability of the nucleus of an atom to attract the electrons involved in a chemical bond.
So the more electronegative, the more partial negative charge the atom will have.
Linus Pauling created a scale of the most electronegative elements, which can be of help in determining the intensity of polarization of different bonds:
F > O > N > C > Br > I > S > C > P > H
In this case, F is the most electronegative element.
So hydrogen will have the greatest partial positive charge bonded to F.
Answer: HF
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients.
Na(s) + O₂(g) → Na₂O₂ (s)
Answer: 2Na(s)+O₂(g) → Na₂O₂ (s)
Explanation: Since there is only one sodium on the left side of the equation and 2 on the right all you have to do is put a 2 in front of the sodium on the left
4. Which atom (magnesium or chlorine) has a higher ionization energy?___________________________(you should also be prepared to answer the question if asked for lower ionization energy)4a. Explain why the atom has a higher ionization energy. Include the definition of ionization energy and the reason why the atom you chose would have a higher value.
Answer:
The Chlorine atom has higher ionization energy.
Explanation:
Ionization energy is the energy needed to separate an electron from an atom of an element in the gaseous state.
In the Periodic Table of Elements, Ionization energy increases from bottom to top (in a group), and increases from left to right (in a period).
In the folowing drawing we can see the variation of the Ionization energy and the location of the magnesium atom and chlorine atom:
Magnesium atom and Chlorine atom are located in the same period, but Mg is in group 2 (left side) and Cl in in group 17 (right side), so the Chlorine atom has higher ionization energy.
Water is a polar solvent; gasoline is a non-polar solvent. Which compound will dissolve in gasoline? Check all that apply.
CCl4
NaCl
NaOH
KCl
Answer:
[tex]\blue{\boxed{\red{\sf CCl_4 \: will \: dissolve \: in \: gasoline}}}[/tex]
Explanation:
The simple concept that would be applied is
'Like Dissolves Like.'
According to this, the polar solvent will dissolve the polar solutes and the non-polar solvent will dissolve the non-polar solutes.
classification of given compounds as polar or non-polar,
[tex]\begin{gathered}\boxed{\begin{array}{c|c} \bf Polar & \bf Non-polar \\ \\ \frac{\qquad \qquad}{} & \frac{\qquad \qquad}{} \\ \sf NaCl & \sf CCl_4 \\ \\ \sf NaOH & \sf - \\ \\ \sf KCl & \sf - \end{array}} \\ \end{gathered}[/tex]
Also, the given data says water is a polar solvent while gasoline is a non-polar solvent. From all the information we have, we can conclude that CCl4 is the only compound that will dissolve in gasoline.
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How many grams of CO2 are produced if 12 liters of H2O are produced?
Answer
[tex]14653.7181\text{ g }CO_2\text{ }[/tex]Procedure
Considering the following balanced equation.
2CH₃OH + 3O₂ ---> 2CO₂ + 4H₂O
To determine the grams of CO₂ that will be produced, you will first need to get the grams of water produced, then convert the grams of water into moles of water and use the molar proportios to get the moles of CO₂. Lastly, convert the moles of CO₂ into grams.
Additional data:
Dnsity of water = 1 g H₂O=/ of H₂O
CO₂ molar mass = 44.01 g/mol
H₂O molar mass = 18.02 g/mol
Calculations
Convert to mass
[tex]12L\text{ }H₂O\text{ }\frac{1kg\text{ }H_2O}{1L\text{ }H_2O}=12kg\text{ }H_2O[/tex]Convert to moles
[tex]12kg\text{ }H₂O\text{ }\frac{1000g\text{ }H_2O\text{ }}{1kg\text{ }H_2O}\frac{\text{ }1\text{ }mole\text{ }H_2O}{18.02g\text{ }H_2O}=665.9267\text{ }mole\text{ }H_2O[/tex]Convert to moles of CO₂ using the relationship
[tex]665.9267\text{ }mole\text{ }H_2O\frac{2moleCO_2}{4mole\text{ }H_2O}=332.9634\text{ }mole\text{ }CO_2[/tex]Convert to grams of CO₂
[tex]332.9634\text{ }mole\text{ }CO_2\text{ }\frac{44.01g\text{ }CO_2}{1\text{ }mole\text{ }CO_2}=14653.7181\text{ g }CO_2\text{ }[/tex]Which of the following formulas represent valid ionic compounds that can be made from these six elements: Al, Be, F, Li, N, and S? Select all that apply. A. AlN B. BeS C. AlLi D. LiF
The compound AlN, BeS, and LiF represents valid ionic compounds.
Ionic bonding:-
When all of the electrons are successfully transferred from one element to another, this sort of bonding is created. One element in this bonding is always a metal, whereas the other is invariably a non-metal.Thus, Al, Be, Li are metals and F, N, S are nonmetals which can form ionic bonding with each other. So, AlLi (Option C) rules out.Considering option A: - AlNThe valency of aluminum is 3 and nitrogen is of 3. The valency of the cations and the anions must be switched and subscripted in order to identify the ionic compound. Thus,Al N
3 3
Simplest ratio : - 1 1
AlN is an ionic compound and thus it is a valid ionic compound.The valency of beryllium is 2 and sulfur of 2. The valency of the cations and the anions are switched and put in subscripts to create the ionic compound. Thus,Be S
2 2
Simplest ratio : - 1 1
The ionic compound created is (b) BeS, making it a legitimate ionic compound.Fluorine and lithium both have valencies of 1. The valency of the cations and the anions are switched and put in subscripts to determine the ionic compound. Thus,Li F
1 1
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What is the hydrogen ion and hydroxide ion concentration for a pH of 4.478? Is the solution acid or base?
Answer
The hydrogen ion concentration, [H⁺] is 3.327 x 10⁻⁵ M
The hydroxide ion concentration [OH⁻] is 3.01 x 10⁻¹⁰ M
The solution is acid.
Explanation
pH is a measure of how acidic or basic a solution is. The range goes from 0 - 14, with 7 being neutral. A pH of less than 7 indicates acidity, whereas a pH of greater than 7 indicates a base. pH is really a measure of the relative amount of free hydrogen and hydroxyl ions in the solution.
Since pH of the solution is 4.478, then it means the solution is acid.
The hydrogen ion concentration, [H⁺] of the solution can be calculated using the pH formula.
[tex]pH=-log[H^+][/tex]Substituting pH as 4.478 into the formula, we have
[tex]\begin{gathered} 4.478=-log[H^+] \\ \\ Multiply\text{ }through\text{ }by\text{ }minus\text{ }(-) \\ \\ log[H^+]=-4.478 \\ \\ .[H^+]=10^{-4.478} \\ \\ .[H^+]=3.327\times10^{-5}\text{ }M \end{gathered}[/tex]The hydrogen ion concentration, [H⁺] is 3.327 x 10⁻⁵ M
The relation between the hydrogen ion concentration, [H⁺] and hydroxide ion concentration [OH⁻] is
[tex].[H^+]\times[OH^-]=10^{-14}[/tex]So, substituting [H⁺] as 3.327 x 10⁻⁵ M, we have:
[tex]\begin{gathered} 3.327\times10^{-5}\times[OH^-]=10^{-14} \\ \\ Divide\text{ }both\text{ }sides\text{ }by\text{ }3.327\times10^{-5} \\ \\ \frac{3.327\times10^{-5}\times\times[OH^-]}{3.327\times10^{-5}}=\frac{10^{-14}}{3.327\times10^{-5}} \\ \\ .[OH^-]=3.01\times10^{-10}\text{ }M \end{gathered}[/tex]Hence, the hydroxide ion concentration [OH⁻] is 3.01 x 10⁻¹⁰ M
Define electronegativity.
A neutral atom has high electronegativity. Describe what happens to this atom during ionic bond formation.
No trolls, fake answers, copied answers
Electronegativity is defined as the ability of an element to accept electrons to its shell during a chemical reaction for the formation of a stable bond structure.
What is a neutral atom?A neutral atom is the atom that contains an equal amount of electrons and protons which means that is has a zero net charge. Example is sodium.
Electronegativity is defined as the ability of an element to accept electrons to its shell during a chemical reaction for the formation of a stable bond structure.
During ionic bond formation, the elements involved tries to obtain an octet structure by either donating or accepting electrons.
Alkali metals( such as the neutral element of sodium? have the lowest electronegativities, while halogens have the highest.
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DUE AT 11:59 PLEASE HELP
A student has a calorimeter with 211.7 grams of 20.4 degrees Celsius water contained within it. The student then adds 128.9 grams of 94.2 degrees Celsius water to that calorimeter and stirs. To what maximum temperature will the cold water in the calorimeter rise to?
The maximum temperature the cold water in the calorimeter will rise to is 48.3 °C
How to determine the maximum temperatureThe maximum temperature the cold water can attain can be obtained by calculating the equilibrium temperature. This can be obtained as follow:
From the question given above, the following data were obtained:
Mass of cold water (M) = 211.7 grams Temperature of cold water (T) = 20.4 °CMass of warm water (Mᵥᵥ) = 128.9 gramsTemperature of warm water (Tᵥᵥ) = 94.2 °CSpecific heat capacity of the water (C) = 4.18 J/gºC Equilibrium temperature (Tₑ) =?Heat loss = Heat gain
MᵥᵥC(Tᵥᵥ – Tₑ) = MC(Tₑ – T)
Cancel out C
Mᵥᵥ(Tᵥᵥ – Tₑ) = M(Tₑ – T)
128.9 × (94.2 – Tₑ) = 211.7 × (Tₑ – 20.4)
Clear bracket
12142.38 – 128.9Tₑ = 211.7Tₑ – 4318.68
Collect like terms
12142.38 + 4318.68 = 211.7Tₑ + 128.9Tₑ
16461.06 = 340.6Tₑ
Divide both side by 340.6
Tₑ = 16461.06 / 340.6
Tₑ = 48.3 °C
Thus, we can conclude that the maximum temperature is 48.3 °C
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5. 10.1 grams of hydrogen gas is contained in a volume of 5.00 L at a temperature of 37.5℃. Find the pressure of the gas.
Answer: 2607.31 pa
Explanation:
n = 10.1/2 = 5.05 mol
Now, according to ideal gas equation,
PV = nRT
⇒ P × 5 = 5.05 × 8.314 × (37.5 +273)
⇒P = 2607.31 Pa
metal oxide MO2 reacts with excess HCl to produce chlorine gas at STP as given by the following unbalanced equation:MO2 (s) + HCl (aq) -,> MCl2 (aq) + Cl2 (g) + H20 (l) a. determine limiting reactantb. calculate the mass of MCl2 produced in the reactionc. calculate the percentage yield if the actual mass of MCl2 produced is 0.078g
1st) It is necessary to balance the chemical equation:
[tex]MO_2+4\text{HCl}\rightarrow MCl_2+Cl_2+2H_2O[/tex]2nd)
