Question

Sample of the oxygen gas and xenon gas are added to an evacuated contained of fixede volume and the following reaction occurs forming a yellow solid:

Xe(g) +2 O_{2(g) --->} 2 O₂ (g) -----> XeO₄ (s)

the initial pressure of oxygen gas is 2.0 atm and that of the xenon gas is 0.7 atm. After the reaction has gone to completion, what is the total pressure inside the container? The temperature remained constant.

Please show me how to solve this problem using I-C-E method in step_by step. Thanks.

Answer 1

Solution:-

Then given balanced equation is...

Xe(g) + 2O₂(g) -------->XeO₄(s)

From balanced equation there is 1:2 mol ratio between Xe and O₂. They would react in the same pressure ratio also. Xe is the limiting reactant. The ice table could be made as...

Xe(g) + 2O₂(g) -------->XeO₄(s)

I 0.7 atm 2.0 atm 0

C -0.7 atm -2(0.7) atm 0

E (0.7 - 0.7)atm (2 - 1.4) atm 0

So, at equilibrium, pressure of Xe(g) = 0

pressure of O₂ = (2 - 1.4) atm = 0.6 atm

Product is the solid so it's pressure would be zero.

Hence, the total pressure after the reaction has gone to completion is 0.6 atm.