10.0 ml of a 0.100 mol l–1 solution of a metal ion m2+ is mixed with 10.0 ml of a 0.100 mol l–1 solution of a substance l. the following equilibrium is established:
m2+(aq) + 2l(aq) picture ml22+(aq)
at equilibrium the concentration of l is found to be 0.0100 mol l–1. what is the equilibrium concentration of ml22+, in mol l–1?
someone me

The concentration of at equilibrium is 0.045 M.

Explanation:

We are given:

For the given chemical equation:

Initially:             0.100M        0.100M

At eqllm:          0.100 - x      0.100 - 2x          x

We are also given:

Equating the two values:

Hence, the concentration of at equilibrium is 0.045 M.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.