HW 11.43

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Hannah Guo 3D
Posts: 56
Joined: Fri Sep 29, 2017 7:06 am

HW 11.43

Postby Hannah Guo 3D » Tue Nov 28, 2017 10:16 pm

11.43 Consider the reaction 2 NO(g) <---> N2(g) + O2(g). If the initial partial pressure of NO(g) is 1.0 bar, and x is the equilibrium concentration of N2(g), what is the correct equilibrium relation? (a) K = x^2/(1.0 - x); (b) K = x^2; (c) K = x^2/(1.0 - 2x)^2; (d) K = 4x^3/(1.0 - 2x)^2; (e) K = 2x/(1.0 - x)^2.

The correct answer is C, but can we use pressure and concentration together in one equation to calculate K? I thought when we use partial pressure of one of the products to calculate K, we need to use partial pressure of the rest of the chemicals. Please explain. Thank you!

Rita Dang 3D
Posts: 31
Joined: Fri Sep 29, 2017 7:07 am

Re: HW 11.43

Postby Rita Dang 3D » Tue Nov 28, 2017 10:21 pm

Professor Lavelle just updated the solution manual errors.
It should be "x is the equilibrium partial pressure."

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