Hey guys, I’m not really sure if I’m doing this right. The questions are:(adsbygoogle = window.adsbygoogle || []).push({});

Equilibrium equations can be written directly from the balanced chemical equation. Check your textbook if you don’t know how. Then write equilibrium constant expressions for the following reactions.

[tex] \begin{array}{l}

a)CO_{(g)} + H_2 O_{(g)} \Leftrightarrow CO_2 _{(g)} + H_{2(g)} \\

b)N_{2(g)} + O_{2(g)} \Leftrightarrow 2NO_{(g)} \\

\end{array} [/tex]

So are these the equations?

[tex]\begin{array}{l}

\frac{{[CO_2 ][H_2 ]}}{{[CO][H_2 ]}} \\

\frac{{[NO]^2 }}{{[N_2 ][O_2 ]}} \\

\end{array}[/tex]

It also asks me …

In what direction, if any, would the equilibrium be shifted if the following changes were done to the above reactions

1) CO2 is added to reaction 1

2) Nitrogen gas is removed from reaction 2

I don’t really understand the 2nd part. How do I determine what to do?

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# Homework Help: Equilibrium equations

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