Question

nitrogen and water react to form nitrogen monoxide and hydrogen, like this:

$n_{2}(g)+2h_{2}o(g)\to2no(g)+2h_{2}(g)$

also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition:

calculate the value of the equilibrium constant $k_{c}$ for this reaction. round your answer to 2 significant digits.

$k_{c}=\square$

Explanation:

Step1: Write the equilibrium constant expression

For the reaction \(N_{2}(g)+2H_{2}O(g)\to2NO(g) + 2H_{2}(g)\), the equilibrium constant \(K_{c}=\frac{[NO]^{2}[H_{2}]^{2}}{[N_{2}][H_{2}O]^{2}}\)

Step2: Substitute the equilibrium concentrations

Given \([N_{2}]=0.43M\), \([H_{2}O]=2.0M\), \([NO]=2.0M\), \([H_{2}]=1.5M\)

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Step3: Calculate the value

\(K_{c}\approx5.2\)

Answer:

\(5.2\)