Question

1. Consider the following reaction:
CO(g)+2H2(g)⇌CH3OH(g)
A reaction mixture in a 5.25 −L flask at a certain temperature contains 26.8 g CO and 2.35 g H2. At equilibrium, the flask contains 8.64 g CH3OH.

Part A

Calculate the equilibrium constant (Kc) for the reaction at this temperature.

2. Consider the following reaction:
CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kp=0.0611 at 2000 K
A reaction mixture initially contains a CO partial pressure of 1358 torr and a H2O partial pressure of 1764 torr at 2000 K.

Part A

Calculate the equilibrium partial pressure of CO2.

Part B

Calculate the equilibrium partial pressure of H2.

3.A system at equilibrium contains

I2(g) at a pressure of 0.13 atm and I(g) at a pressure of 0.18 atm . The system is then compressed to half its volume.

Part A

Find the pressure of I2 when the system returns to equilibrium.

Part B

Find the pressure of I when the system returns to equilibrium.

Please HELP!

Answer 1