predict whether each of the following pressure changes would favor forward reaction or reverse reaction...?

Question

2NO(g) + O2(g) <--> 2NO2(g)

A-increased pressure
B-decreased pressure

Answer 1

when u increase the pressure of one of the elements on the left side of the equation, the arrow goes to the left coz it needs to balance the pressure on both sides so it needs to take away the extra pressure.

same thing happens when u decrease the pressure when u decrease the pressure of one of the elements on the left side of the equation, the arrow goes to the left coz it needs to give the elements more pressure.

the arrow goes to the right when one of the elements on the right of the equation is increased or decreased.

Answer 2

Let's assume that you are either decreasing the volume of the container (increasing pressure) OR increasing the volume of the container (decreasing pressure) .

If you were to decrease the container volume, the reaction would shift toward the side with fewer moles of gas. In this case, that would be a shift to the right.

If, instead, the container volume is increased, the reaction equilibrium will shift to the side that has the larger number of moles of gas. In this case, increasing the container volume would cause a shift toward the left (because 3 moles of gas take up a larger volume than 2 moles of gas)

So A-increased pressure causes a shift toward the right.

B-decreased pressure causes a shift toward the left.

Hope that was helpful.

Answer 3

Higher pressure pushes the reaction from the side that has more moles to the side that has fewer moles.

Lower pressure does the opposite.

Count up the coefficients in your reaction and it is easy to see the answer.