Question

Nitrogen and oxygen react to form nitrogen monoxide, like this:

N2 (g) +O2 (g) ->2NO (g)
The reaction is endothermic. Suppose a mixture of N2, O2 and NO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left.

Answer 1

A catalyst is added to the reaction vessel will the pressure of N2 go up, go down or neither? Will it shift in equilibrium? to right, to left or neither?
If the temperature is raised will the pressure of N2 go up, go down or neither? Will it shift in equilibrium? to right, to left or neither?
A catalyst is added to the reaction vessel will the pressure of NO go up, go down or neither? Will it shift in equilibrium? to right, to left or neither?
If the temperature is raised will the pressure of NO go up, go down or neither? Will it shift in equilibrium? to right, to left or neither?

Answer 2

A condition in which a chemical reaction is occurring at equal rates in, an acid and a base react to form water and a salt, that is a true chemical reaction. Of matter for the reactants and products: (s) for a solid; (l) for a liquid; (g) for a gas. In any case, no change in volume alters the equilibrium constant also

Answer 3

lower the pressure, the equilibrium shift if more H2 is added to this reaction at equilibrium. In order to do this, the reaction must shift to the left.

Answer 4

H2? The question only lists N2 and NO. So does that mean that none of it changes?

Answer 5

You got that right.

Answer 6

So the equilibrium stays the same with all variables is that correct?

Answer 7

Correct

Answer 8

Cool, thanks!

Answer 9

Your Welcome