# Consider this equilibrium: n2(g) + o2(g) 2no(g).nitrogen gas and oxygen gas react when placed in a closed

Consider this equilibrium:
n2(g) + o2(g) 2no(g).
nitrogen gas and oxygen gas react when placed in a closed container. as the reaction proceeds towards equilibrium, what happens to the rate of the reverse reaction? it increases as the concentration of products decreases.
it decreases as the concentration of products decreases.
it increases as the concentration of products increases.
it decreases as the concentration of products increases.
it remains constant as the concentration of products remains constant.

## This Post Has 3 Comments

1. tdahna0403 says:

Consider this equilibrium:
N2(g) + O2(g) 2NO(g).

Nitrogen gas and oxygen gas react when placed in a closed container. As the reaction proceeds towards equilibrium, what happens to the rate of the reverse reaction?
1It increases as the concentration of products decreases.
2It decreases as the concentration of products decreases.
3It increases as the concentration of products increases.
4It decreases as the concentration of products increases.
5It remains constant as the concentration of products remains constant.

C

2. donuteatingcat says:

It is C). It decreases as the concentration of products increases.

3. kassidy49 says:

It decreases as the concentration of products decreases.

It increases as the concentration of products increases.

Explanation:

the equilibrium reaction is

$N_{2}(g)+O_{2}(g)<==2NO(g)$

As per equilibrium,

a) there will be no effect of pressure change on the equilibrium as the number of gaseous molecules are same on both the side of reaction.

b) there will be no effect of addition of inert gas on the equilibrium as the number of gaseous molecules are same on both the side of reaction.

c) the reverse reaction rate can be increased by

i) decreasing the concentration of reactants

ii) increasing the concentration of products