11.43 in 6th Edition

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Janice Park 1E
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Joined: Fri Sep 28, 2018 12:22 am

11.43 in 6th Edition

Postby Janice Park 1E » Sat Jan 12, 2019 9:16 pm

In the 6th edition of the textbook, the question says:

Consider the reaction 2 NO(g) Δ 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?

When solving this question, does it not matter if we use partial pressure for NO and concentration of N2? Should we convert one to pressure or the other to concentration? Additionally, is it safe to assume that the other concentrations are initially 0 when worded like this?

Matthew Choi 2H
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: 11.43 in 6th Edition

Postby Matthew Choi 2H » Sat Jan 12, 2019 11:44 pm

You should probably convert one of them to the other. And yes, it's usually safe to assume the starting concentration/partial pressures of the products are 0 if not explicitly stated.

Iris Bai 2K
Posts: 60
Joined: Fri Sep 28, 2018 12:18 am

Re: 11.43 in 6th Edition

Postby Iris Bai 2K » Sun Jan 13, 2019 2:06 am

I would complete the ICE table using partial pressures and convert your answer to molar concentrations afterwards.


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