Exercise 17.70 Use data from Appendix IIB to calculate the equilibrium constants

Question

Exercise 17.70

Use data from Appendix IIB to calculate the equilibrium constants at 25 ?C for each of the following reactions..

Part A

N2(g)+3H2(g)?2NH3(g)

Express your answer using two significant figures.

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Part B

Br2(g)+Cl2(g)?2BrCl(g)
?G?f for BrCl(g) is -1.0 kJ/mol

Express your answer using two significant figures.

PROBLEM #2

Relationship between free energy and the equilibrium constant

The standard free energy change, ?G?, and the equilibrium constant K for a reaction can be related by the following equation:

?G?=?RTlnK

where T is the Kelvin temperature and R is equal to 8.314 J/(mol?K).

Part B

Calculate the equilibrium constant for the following reaction at room temperature, 25 ?C:

N2(g)+O2(g)?2NO(g)

Express your answer numerically to three significant figures.

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Explanation / Answer

N2(g)+3H2(g)?2NH3(g)

Express your answer using two significant figures.

K =

First find delta G by doing products - reactants

=
delta G = 2* (16.4) – 3(0)

delta G = -32.8 kJ/mol

or = -32800 J/ mole
delta G = -RT lnK

lnK = - delta G /RT

K= e^ - (-32800) /8.3145 *298
=e ^13.24
K = e^(16.48) = 5.62x10^5

Part B

Br2(g)+Cl2(g)?2BrCl(g)
?G?f for BrCl(g) is -1.0 kJ/mol

First find delta G by doing products - reactants

=
delta G = 2* (-1) – (0) – 3.14

delta G = -5.14 kJ/mol

or = -5140 J/ mole
delta G = -RT lnK

lnK = - delta G /RT

K= e^ - (-5140) /8.3145 *298
=e ^2.075
K = e^(2.075) = 7.96

K =

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