Question

Given the following reaction:
3 H2(g) + N2(g) <- -> 2NH3(g) + heat

If the following changes were to occur what direction shift will it have (left or right)
And what will be the reason of the shift

Changes/Stress on system:
Adding NH3
Decreasing the pressure
Adding heat
Removing N2
Increasing the pressure

Answer 1

In common words, Le Chatelier's Principle tells us that when a system in equilibrium is subjected to a stress, it will shift to undo what we did to it.
So look at the equation.
3 H2(g) + N2(g) <- -> 2NH3(g) + heat


Adding NH3. So the reaction will try to use up NH3 to get rid of what we added. How can it do that? Shift to the left.

When increasing P, the reaction shifts to the side with fewer mols.

See if you can finish.

Answer 2

so when you increase p does that mean it shifts to the left

Answer 3

No i think its to the right

Answer 4

That's right. Increasing P shifts to the side with fewer mols OF GAS. There are 4 mols on the left and 2 on the right so increasing P shifts to the right; decreasing P shifts it to the left.