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Rudiy27
3 years ago
5

The heat of vaporization, ΔHvap of carbon tetrachloride (CCl4) is 43000 J/mol at 25 °C. 1 mol of liquid CCl4 has an entropy of 2

14 J/K. (a) What is the entropy of 1 mole of the vapor at 25 °C or 298 K? (b) How many intensive variables will be required to completely specify the vapor-liquid mixture of CCl4? (45 points)
Chemistry
1 answer:
Alexxandr [17]3 years ago
7 0

Explanation:

(a)    The given data is as follows.

     Temperature (T) = 25^{o}C = (25 + 273) K = 298 K

      \Delta H_{vap} = 43000 J/mol

Since, both the liquid and vapors are at equilibrium. Therefore, change in free energy will be calculated as follows.

      \Delta G_{vap} = \Delta H_{vap} - T \Delta S_{vap} = 0        

            43000 - (298 \times \Delta S_{vap}) = 0

                      \Delta S_{vap} = -144 J/mol K

Negative sign indicates an increase in entropy of the system.

Now, for 1 mole of CCl_{4} is as follows.

     = 144 J/K

So,     S_{vapor} - 214 = 144 J/k

                         = 358 J/K

Therefore, we can conclude that entropy of CCl_{4} vapor is 358 J/K.

(b)  As we know that intensive variable are the variables which do not depend on the amount of a substance.

So, in the given situation only temperature will act as an intensive variable that will be required to completely specify the vapor-liquid mixture of CCl_{4}.

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kodGreya [7K]

Answer : The rate law for the overall reaction is, Rate=k[A][B]

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

As we are given the mechanism for the reaction :

Step 1 : A+B\rightarrow AB    (slow)

Step 2 : A+AB\rightarrow A_2B     (fast)

Overall reaction : 2A+B\rightarrow A_2B

The rate law expression for overall reaction should be in terms of A and B.

As we know that the slow step is the rate determining step. So,

The slow step reaction is,

A+B\rightarrow AB

The expression of rate law for this reaction will be,

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Hence, the rate law for the overall reaction is Rate=k[A][B]

3 0
3 years ago
In this stoichiometry problem, determine the limiting reactant.
Tanya [424]

Answer:

Limiting reactant is NiSO₄

Explanation:

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<em>That means 2 moles of Al react with 3 moles of nickel sulfate.</em>

<em />

Moles of Al and NiSO₄ are:

Al: 108g × (1mol / 26.98g) = 4.00 moles of Al

NiSO₄: 464g × (1mol / 154.75g) = 3.00 moles of NiSO₄

For a complete reaction of aluminium there are necessary:

4.00mol Al ₓ ( 3 moles NiSO₄ / 2 moles Al) = 6 moles of NiSO₄

As you have just 3.00 moles of NiSO₄, the <em>limiting reactant is NiSO₄</em>

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3 years ago
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JulijaS [17]

Answer:

D. chlorine, oxygen, nitrogen, hydrogen.

Explanation:

  • Thomas Graham found that, at a constant  temperature and pressure the rates of effusion  of various gases are inversely proportional to  the square root of their masses.

<em>ν ∝ 1/√M</em>

where ν is the rate of effusion and M is the atomic  or molecular mass of the gas particles.

  • The molecular mass for the listed gases are:

O₂: 32.0 g/mol,

Cl₂: 70.906 g/mol,

N₂: 28.0 g/mol,

H₂: 2.0 g/mol.

  • Hence, the smallest molecular mass of the gas, the fastest rate of effusion.

So, the order from the slowest to the fastest rate of effusion is:

<em>Chlorine, oxygen, nitrogen, hydrogen.</em>

6 0
3 years ago
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Answer:

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vlabodo [156]

Answer:

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Explanation:

I just learned this in science.

I hope this helps!

7 0
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