Answer: valeraldehyde
Explanation:
I had to memorize this one
The functional group present is aldehyde and name of compound is valeraldehyde.
What are functional groups?Functional group is defined as a substituent or group of toms or an atom which causes chemical reactions.Each functional group will react similarly regardless to the parent carbon chain to which it is attached.This helps in prediction of chemical reactions.
The reactivity of functional group can be enhanced by making modifications in the functional group .Atoms present in functional groups are linked to each other by means of covalent bonds.They are named along with organic compounds according to IUPAC nomenclature.
Functional group inter conversion is also possible by retro -synthesis.In some cases , functional groups can be charged molecules.
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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
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]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
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]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
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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Define hydrogen bonding and explain how hydrogen are bonding involved in the
transfer of genetic material.
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:
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.
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
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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Tablet salt (sodium chloride) is an example of a(n): A) element B) compound C) mixture
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.
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.
(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.
How many moles of H2 is needed to produce 12 moles of NH3
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
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.
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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The energy released when a nucleus forms is calledQuestion 26 options: enthalpy. atomic mass. a becquerel. binding energy.
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.
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:
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]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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30.Vegetable soup is classified as which of the following?Select one:a. An atom.b. A compound.c. An element.d. A mixture.
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
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℃?
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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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
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
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%.
What is a molecular equation and what is this question asking please help?
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
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]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
4. Collaborate with a partner, make a brochure that highlights an example of a
technology that you have seen in which density is important.
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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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.
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
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]
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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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.
Answer:2ZnO(s)→2Zn(l)+O2(g)
Explanation:
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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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
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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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
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
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
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.
