For the reaction co(g) + 3 h2(g) ⇌ h2o(g) + ch4(g), kc = 189 at 1000 k. if a vessel is filled with these gases such that the initial concentrations are [co] = 0.0360 m, [h2] = 0.0450 m, [h2o] = 0.0200 m, and [ch4] = 0.0310 m, in which direction will a reaction occur and why?

There will be no change since Qc = Kc

Explanation:

Given:

[CO] = 0.0360 M

[H2] = 0.0450 M

[H2O] = 0.0200 M

[CH4] = 0.0310 M

Kc = 189

To determine:

The direction in which the given reaction will occur

Calculation:

The given reaction is:

The relation between the equilibrium constant Kc and the reaction quotient Qc determines the reaction direction

If Qc > Kc reaction will shift to the left

If Qc < Kc reaction will shift to the right

If Qc = Kc there will be no shift

Based on equation (1), for the given reaction:

Since Qc=Kc, there will be no change in the reaction direction and the equilibrium will be retained

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.

it is b that is the answer.