Question

The reaction shown here occurs inside a closed flask.NO2(g) + CO(g) → NO(g) + CO2(g)What action will shift the reaction to the left?→Pumping CO gas into the closed flaskRaising the total pressure inside the flaskVenting some CO2 gas from the flaskIncreasing the NO concentration in the flask

Answer 1

increasing the NO concentration in the flask will shift the reaction to the left

option D

Step-by-step explanation

Given that

`\text{ NO}_(2(g))\text{ + CO}_((g))\rightleftarrows\text{ NO}_((g))\text{ + CO}_((2)(g))`

To identify the direction of the equilibrium, follow the steps below

Step 1: State Le Chatelier's principle

Le Chatelier's principle state that when an external constraint such as temperature, pressure, or concentration is imposed on a chemical equilibrium system, the equilibrium arrow will adjust so as to annul the effect of the constraint.

Looking at the reaction, you will see that the number of moles of reactants is equal to the number of moles of the products. Hence, pressure will not have effect on the reaction.

Since the reaction is a reversible reaction, the products and reactants are produced simultaneously.

Therefore, adding more of the products will favor the production of the reactants ( favors the reverse reaction)

Hence, increasing the NO concentration in the flask will shift the reaction to the left