For each event, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. A

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For each event, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. A

n up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. 2 CO ( g ) 2CO(g) + + O 2 ( g ) O2(g) − ⇀ ↽ − ↽−−⇀ 2 CO 2 ( g ) 2CO2(g) increasing the concentration of CO CO increasing the concentration of CO 2 CO2 decreasing the volume of the system ↑ ↑ ↑ ↑ ↓ ↓ ↓ ↓ ↓ ↓ ↑ ↑ ↓ ↓ ↓ ↓ ↑ ↑

Chemistry

1 answer:

const2013 [10] · Answer 1 · 2023-04-29T22:32:13+03:00

Answer:

1. Increasing concentration of CO:

The concentration of the product, CO₂(g) increases (↑) and the concentration of the reactants, CO(g) and O₂(g) decreases (↓)

2. Increasing concentration of CO₂:

The concentration of the reactants, CO(g) and O₂(g) increases (↑) and the concentration of the product, CO₂(g), decreases (↓).

3. Decreasing the volume of the system:

The concentration of the product, CO₂(g) increases (↑) and the concentration of the reactants, CO(g) and O₂(g) decreases (↓).

Explanation:

According to the Le Chatelier's principle, for a given chemical reaction at equilibrium, a change in the concentration of any chemical species or volume causes the equilibrium of the reaction to shift in a direction, that minimizes the effect of the change.

Given reaction: 2CO(g) + O₂(g) ⇌ 2CO₂(g)

1. Increasing concentration of CO:

When the concentration of the reactant CO(g), increases; the equilibrium shifts towards the forward direction or product side, thereby increasing the concentration of the product, CO₂(g) and decreasing the concentration of the reactants, CO(g) and O₂(g).

2. Increasing concentration of CO₂:

When the concentration of the product CO₂(g), increases; the equilibrium shifts towards the backward direction or reactant side, thereby increasing the concentration of the reactants, CO(g) and O₂(g) and decreasing the concentration of the product, CO₂(g).

3. Decreasing the volume of the system:

When the volume of the system decreases, the pressure increases, thus causing the equilibrium of the reaction to shift in a direction that produces less number moles of gas.

Since, total number of moles of gaseous reactants and products is 3 and 2, respectively.

Therefore, when the volume of the system decreases; the equilibrium of the reaction shifts towards the forward direction or product side, thereby increasing the concentration of the product, CO₂(g) and decreasing the concentration of the reactants, CO(g) and O₂(g).