# Problem: At 700 K, the reaction below has a Kp value of 54. An equilibrium mixture at thistemperature was found to contain 1.84 atm of I2 and 4.24 atm of HI. Calculate the equilibrium pressure of H2.H2(g) + I2(g) &lt;=&gt; 2 HI(g).  Enter answer to 2 decimal placesA. 0.18 atmB. 0.04 atmC. 5.53 atmD. 0.30 atmE. 0.81 atm

###### FREE Expert Solution

We’re being asked to determine the equilibrium concentration of H2 at 700 K for the following reaction:

H2(g) + I2(g)  2 HI(g)

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

We use Kp when dealing with pressure and Kc when dealing with concentration:

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

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

###### Problem Details

At 700 K, the reaction below has a Kp value of 54. An equilibrium mixture at this
temperature was found to contain 1.84 atm of I2 and 4.24 atm of HI. Calculate the equilibrium pressure of H2.

H2(g) + I2(g) <=> 2 HI(g).  Enter answer to 2 decimal places

A. 0.18 atm
B. 0.04 atm
C. 5.53 atm
D. 0.30 atm
E. 0.81 atm