Question

Ammonium bromide is a crystalline solid that decomposes endothermically when heated:

NH4Br(s) ⇌NH3(g) + HBr(g). When solid NH4Br is added to an evacuated flask at 300 °C, which change in reaction conditions below will cause the equilibrium to shift to the right?

A) add more NH3

B) add more NH4Br

C) decrease the temperature

D) double the volume of the container

Answer 1

B) add more NH₄Br

Explanation:

The reaction equation is given as:

                      NH₄Br → NH₃ + HBr

In the reaction above, when more NH₄Br is added, the equilibrium position will shift to the right hand side of the equation. This implies that more products will be produced.

• Le Chatelier's principle states that "if any of the conditions of a system in equilibrium is changed, the system will adjust itself in order to annul the effect of the change".
• Adding more NH₄Br in this endothermic reaction is increasing the concentration of the reactant.
• The system will shift the equilibrium to the right by trying to establish a balance between the products and the reactants.

Learn more:

chemical equilibrium https://brainly.com/question/2396642

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Answer 2

Answer:

Doubling the volume of the container

Explanation:

when V increases so does the number of moles, then the reaction will shift while trying to offset.