Multiple Choice
What is the value of Kp for the reaction 2 SO3(g) ⇌ 2 SO2(g) + O2(g) if the equilibrium partial pressures are P(SO3) = 0.2 atm, P(SO2) = 0.4 atm, and P(O2) = 0.1 atm?
16. Chemical Equilibrium
Equilibrium Constant K
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How can the reverse equilibrium constant for the reaction 8 H₂(g) + 8 Br₂(g) ⇌ 16 HBr(g) be expressed?
A
K
B
K⁻²
C
K²
D
1/K
Verified step by step guidance1
Identify the given chemical reaction: 8 H₂(g) + 8 Br₂(g) ⇌ 16 HBr(g).
Understand that the equilibrium constant (K) for a reaction is expressed as the ratio of the concentrations of the products to the reactants, each raised to the power of their stoichiometric coefficients.
For the forward reaction, the equilibrium constant expression is: K = ([HBr]^{16}) / ([H₂]^{8} [Br₂]^{8}).
To find the reverse equilibrium constant, you need to take the reciprocal of the forward equilibrium constant. This is because reversing a reaction inverts the equilibrium constant.
Thus, the reverse equilibrium constant is expressed as 1/K, which corresponds to the reciprocal of the forward reaction's equilibrium constant.
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