🤓 Based on our data, we think this question is relevant for Professor TBA's class at UBC.

We’re being asked to **determine the equilibrium constant** at 458 ˚C for **this reaction**:

H_{2}(g) + I_{2}(g) ⇌ 2 HI(g)

Recall that the ** equilibrium constant** is the ratio of the products and reactants.

We use **K _{p}** when dealing with pressure and

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}}$ $\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{\left[}\mathbf{products}\mathbf{\right]}}{\mathbf{\left[}\mathbf{reactants}\mathbf{\right]}}}$

*Note that solid and liquid compounds are ignored in the equilibrium expression.*

An equilibrium mixture of H_{2}, I_{2 }and HI at 458°C contains 1.34 atm of H_{2}, 1.34 atm of I_{2} and 9.30 atm of HI.

What is the equilibrium constant (K_{p}) for this reaction?

a) 31.6

b) 48.2

c) 64.7

d) 78.3

e) 92.5

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