Multiple Choice
Which of the following reactions has K_p equal to K_c at all temperatures?
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16. Chemical Equilibrium
Kp and Kc
Multiple Choice
For which reaction(s) will Kp = Kc?
a) N2(g) + O2(g) ⇌ 2 NO(g)
b) CaCO3(s) ⇌ CaO(s) + CO2(g)
c) 2 CH4(g) ⇌ C2H2(g) + 3 H2(g)
d) H2O(g) + CO(g) ⇌ H2(g) + CO2(g)
A
a) only
B
b) only
C
c) only
D
d) only
E
a) and d)
F
b) and c)
Verified step by step guidance1
Understand the relationship between Kp and Kc. Kp is the equilibrium constant for gases expressed in terms of partial pressures, while Kc is expressed in terms of concentrations. The relationship between Kp and Kc is given by the equation: , where Δn is the change in moles of gas.
Calculate Δn for each reaction. Δn is the difference between the moles of gaseous products and the moles of gaseous reactants. For reaction a) , for reaction b) , for reaction c) , and for reaction d) .
Identify when Kp equals Kc. Kp equals Kc when Δn equals zero because the term becomes 1, making Kp = Kc.
Apply the condition to each reaction. For reaction a) and d), Δn is zero, so Kp = Kc. For reaction b) and c), Δn is not zero, so Kp ≠ Kc.
Conclude which reactions have Kp = Kc. Based on the calculations, reactions a) and d) have Kp = Kc because their Δn is zero.
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