I have the following problem I am stuck on, specifically the last bit (iii). The first parts are fairly trivial and I have arrived at the following equation to determine the temperature:

$$T=\frac{\Delta H}{\Delta S - R \ln K}$$

However I am unsure on how to proceed. I do not have a value for $K_p$ and I can't think of how to deduce it. I have tried the following, by assuming that $n_{\ce{Fe3O4}}=n_{\ce{CO}}$, going to the following expression

$$K = \frac{(0.9 x)^3 (0.9 x)}{(0.1x)(0.1x)}$$

but obviously that doesn't cancel.

Any help? I'm probably barking up the wrong tree with the above expression as I'm aware I'm looking for $K_p$ in terms of partial pressures but it would surely result in the same overall problem.


  • $\begingroup$ Just out of curiosity, where is this question from? $\endgroup$ Apr 20, 2016 at 19:14

1 Answer 1


Assuming $\ce{FeO}$ and $\ce{Fe3O4}$ are solid throughout the range of temperatures we are interested in, they won't appear in the expression for the equilibrium constant $K$ (which in this case is equivalent to $K_p$). If $n$ is the total number of moles of $\ce{CO}$ that you start with,

$$K_p = K = \frac{p_{\ce{CO2}}}{p_{\ce{CO}}} = \frac{n_{\ce{CO2}}}{n_{\ce{CO}}} = \frac{0.9 n}{0.1 n} = 9$$

Plugging this into the formula previously derived, we find $T = 1388~\mathrm{K}$.

  • $\begingroup$ Indeed, although I'm not sure how you reached a value of ~1800 K, I think this is the correct answer. On a side note - please visit this page, this page and this ‎one on how to format your future posts better with MathJax and Markdown. I'll help you edit it this time. $\endgroup$ Apr 20, 2016 at 19:24
  • $\begingroup$ The question is from the 2014 exam paper for the IA (First year undergrad) Chemistry course at Cambridge Uni. $\endgroup$
    – Sam
    Apr 20, 2016 at 21:16
  • $\begingroup$ Indeed, I thought so. $\endgroup$ Apr 20, 2016 at 21:34

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