# Problem: At a given temperature, 3.7 atm of H2 and 1.09 atm of Br2 are mixed and allowed to come to equilibrium. The equilibrium pressure of HBr is found to be 1.088 atm. Calculate Kp for the reaction at this temperature.H2(g) + Br2(g) &lt;=&gt; 2 HBr(g).  Use 3 decimal places.A. 226.597B. 0.293C. 0.687D. 208.269E. 0.631

###### FREE Expert Solution

We are being asked to calculate Kp for the given reaction:

H2(g) + Br2(g) 2 HBr(g)

When dealing with equilibrium and Kp:

Kp → equilibrium units in terms of pressure
Kp is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the pressures in the equilibrium expression

Given:

###### Problem Details

At a given temperature, 3.7 atm of H2 and 1.09 atm of Br2 are mixed and allowed to come to equilibrium. The equilibrium pressure of HBr is found to be 1.088 atm. Calculate Kp for the reaction at this temperature.

H2(g) + Br2(g) <=> 2 HBr(g).  Use 3 decimal places.

A. 226.597
B. 0.293
C. 0.687
D. 208.269
E. 0.631