Question

The reaction CO(g)+2H2(g) CH_2OH(g) has delta Hdegree=-18kj. How will the amount of CH_3OH present at equilibrium be affected be affected by the following? Adding CO(g) Removing H_2(g) Decreasing the volume of the container Adding a catalyst Increasing the temperature

Answer 1

CO + 2H2 -----> CH3OH deltaH = -18KJ

1. Adding of CO: If concentration of molecules on left side increases, equiibrium shifts to right side & viceversa

Therefore adding of CO, increases the formation of CH3OH

2. Removing H2: If concentration of molecules on left side decreases, equiibrium shifts to left side & viceversa

Therefore removing of H2, decreases the formation of CH3OH

3. decreasing the volume of container: if volume of a reaction decreases, then the equilibrium shifts to the side having least number of moles of molecules and viceversa

therefore, if volume decreases, formation of CH3OH increases

4. Adding a catalyst: No effect on equilibrium

5. Increasing the temperature: if temperature increases, for exothermic reaction equilibrium shifts to backward and for endothermic reaction shifts to forward

therefore, the with increase in temperature formation of CH3OH decreases