Calculate the equilibrium composition for the reaction H2−− 1 2O2 −−)−−* H2O when the ratio of the number of moles of elemental hydrogen to elemental oxygen is unity. Perform this calculation at T = 2000 K and P = 1 atm.

the equilibrium composition Kp is 3471.01

Explanation:

Given;

H₂ + ½O₂ ↔ H₂O

Using Gibb's formula;

---------(i)

where;

ΔG(T) is change in Gibb's energy and it is given as;

= 1(-241,820 + 82,593 -9904 - 2000 x 264.571) - 1(0 + 61,400 - 8468 - 2000 x 188.297) - 0.5(0 + 67,881 -8682 - 2000 x 268.655)

= -698273 + 323662 + 239055.5

= -135,555.5 KJ

Substituting this value into equation (i)

Therefore, the equilibrium composition Kp is 3471.01

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

12 is it do you think so