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Given the equilibrium reaction at constant pressure:
2HBr(g) + 17.4 kcal — H2(g) + Br2(g)
When the temperature is increased, the equilibrium will shift to the
A Right, and the concentration of HBr(g) will increase
B Left, and the concentration of HBr(g) will decrease
C Right, and the concentration of HBr(g) will decrease
D) Left, and the concentration of HBr(g) will increase

Respuesta :

Answer: C Right, and the concentration of HBr(g) will decrease

Since it is an endothermic reaction the equilibrium will shift to the right direction i.e. product side decreasing concentration f HBr.

In the case when the temperature is increased so here the equilibrium should be shifted to the right and the concentration of HBr(g) will decrease.

Impact on increase in temperature:

The given reaction represent the endothermic reaction since it absorb the heat.

So in the case when there is endothermic reaction so here there should be increase in temperature since the reaction should goes forward direction and the concentration of HBr(g) will decrease.

Learn more about temperature here: https://brainly.com/question/2821877

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