Consider this reaction:N2 (g) + 3H2 (g) 2NH3 (g)
What will happen if more hydrogen gas is added to the reaction mixture?
There will be a shift toward the products.
There will be a shift toward the reactants.
There will not be a shift in equilibrium.
The value for Keq will change.

Answers

Answer 1

Answer: The answer is There will be a shift toward the reactants.

To solve this problem, it is necessary to understand Le Chatelier's principle. According to the principle, if a chemical reaction undergoes changes in conditions, the chemical equilibrium will shift in order to undo the effects. In the reaction N2 (g) + 3H2 (g) ⇄ 2NH3 (g), when hydrogen gas is added to the reaction mixture, the concentration of chemicals will increase in the mixture. The system will try to decrease the concentration by removing H2, so the equilibrium will be shifted toward the reactants.

Answer 2

Answer:

Final answer:

If more hydrogen is added, the equilibrium of the reaction will shift towards the products, leading to more production of ammonia to counterbalance the increase in hydrogen. The value for Keq will not change unless the temperature changes.

Explanation:

The reaction in question involves the reactants nitrogen (N2) and hydrogen (H2) combining to form ammonia (NH3). This is a chemical equilibrium process. In chemistry, Le Chatelier's principle states that if you disturb a system at equilibrium, the system will adjust itself to reduce that disturbance.

Therefore, if more hydrogen (one of the reactants) is added, the system will try to reduce it by using more H2 in the reaction to produce more ammonia (NH3)—the product. This shift in equilibrium is an attempt to counteract the increase in concentration of hydrogen. Hence, the equilibrium will shift towards the products. Moreover, the equilibrium constant (Keq) will not change unless the temperature of the system changes, as it is only dependent on temperature not on concentrations of reactants or products.

Learn more about Chemical Equilibrium here:

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