Question

Carbon dioxide and water react to form methane oxygen like this: CO2(g)+2H2O(g)——>CH4(g)+2O2(g)The reaction is endothermic. How was the mixture of CO2, H2O, CH four and O2 has come to equilibrium in a closed reaction vessel. Predict that changed, 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.Perturbation: The temperature is raisedChange in composition:Pressure in the H20 will?Go up, go down, not change.Shift in equilibrium:To the right, to the left, none.Perturbation:The temperature is loweredChange in the composition:The pressure of the CH4 will?Go up, go down, not change.Shift in equilibrium:To the right, to the left, none.

Answer 1

ANSWER

An increased temperature will shift the equilibrium to the right and the pressure of water will be decreased.

A decreased in temperature will shift the equilibrium to the left and the pressure of the

STEP-BY-STEP EXPLANATION:

Firstly, we need to write out the balanced equation of the chemical equation.

$CO_{2(g)}+2H_2O_{(g)}\rightarrow CH_{4_{((g)}}+2O_{2(g)}$

What is chemical equilibrium?

Chemical equilibrium is the condition in the course of a reversible chemical reaction in which no net change in the amounts of reactant and products occurs.

According to the balanced equation, it shows that the reaction is an endothermic reaction. This means that heat was absorbed from the surroundings during the reaction.

To study the change in the equilibrium shift, we need to apply Le Chatelier's principle.

Le Chatelier's principle states that when an external constraint such as (temperature, pressure, or concentration) is imposed on a chemical system in equilibrium, the equilibrium of the system shift in order to annul or neutralize the effect of the constraints.

When the temperature of the chemical system is increased, the products side of the system will be favored. This is because an increase in temperature will lead to a faster collision between the two reactants, hence, producing more methane. Therefore, the equilibrium will shift to the left.

When the temperature is increased, the equilibrium will shift to the right.

The pressure of water will be decreased when the temperature is increased. This is because has no effect on the equilibrium system

When the temperature is lowered, the reactants side is favored and the equilibrium will shift to the left.

Looking at the balanced equation critically, the number of moles at the reactant side is equal to the number of moles at the sides of the product.

When the temperature is lowered, the pressure of methane gas will be decreased