Math

QuestionHow can you increase the formation of Cl2\mathrm{Cl}_{2} in this reaction?
4HCl(g)+O2( g)2H2O(g)+2Cl2( g)+203 kJ 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+2 \mathrm{Cl}_{2}(\mathrm{~g})+203 \mathrm{~kJ}
A. remove HCl\mathrm{HCl} B. increase the volume C. add H2O\mathrm{H}_{2} \mathrm{O} D. cool the system

Studdy Solution

STEP 1

Assumptions1. The reaction is a reversible reaction. . The reaction is exothermic, as indicated by the positive value of heat on the product side.
3. Le Chatelier's principle applies, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

STEP 2

Let's analyze each of the optionsA. Removing HCl According to Le Chatelier's principle, if we remove a reactant, the reaction will shift to the left to replace the removed reactant. This would decrease the production of Cl2.
B. Increasing the volume of the container Increasing the volume of the container causes the reaction to shift towards the side with more gas molecules. In this reaction, there are5 gas molecules on the reactant side and4 on the product side. Therefore, increasing the volume would shift the reaction to the left, decreasing the production of Cl2.
C. Adding H2 Adding a product to the reaction would cause the reaction to shift to the left according to Le Chatelier's principle, to decrease the concentration of the added product. This would decrease the production of Cl2.
. Cooling the system Since the reaction is exothermic, it releases heat. According to Le Chatelier's principle, cooling the system (removing heat) would cause the reaction to shift to the right to replace the heat that was removed. This would increase the production of Cl2.

STEP 3

Based on the analysis in2, the method that would encourage more product, Cl2, to form from the reaction is to cool the system.
The answer is D. Cool the system.

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