In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right?

CO(g) + 3H2 (g)CH4 (g) + H2O (g) H = -206 kJ/mol

decreasing the concentration of carbon monoxide (CO)

increasing the volume of the reaction system

decreasing the concentration of hydrogen gas (H2)

lowering the temperature of the reaction

Question

In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right? 

CO(g) + 3H2 (g)CH4 (g) + H2O (g)  H = -206 kJ/mol

 decreasing the concentration of carbon monoxide (CO)

 increasing the volume of the reaction system

 decreasing the concentration of hydrogen gas (H2)

 lowering the temperature of the reaction

anonymous · Answer

Lowering the temperature i'm pretty sure the rest of them should push the reaction to the left

anonymous · Answer

So would you increase the temperature?

anonymous · Answer

yes Increasing the heat should make the rxn want to give off more heat to keep equilbrium

anonymous · Answer

Okay thank you so much!(:

anonymous · Answer

But since that isnt an option what would you do?

anonymous · Answer

Lowering the temp should be the answer if you add heat as a product it should push right. Adding heat as a reactant should make it push left.

anonymous · Answer

Oh okay(: Thank you for your time