The following reaction is endothermic in the forward direction. NH4Cl(s) <->NH3(

Question

The following reaction is endothermic in the forward direction. NH4Cl(s) <->NH3(g) + HCl(g) For each of the following cases, briefly explain whether the action causes net reaction from left to right, right to left, or no net reaction. Also, state whether the equilibrium partial pressure of NH3 increases, decreases or stays the same. (a) increasing the temperature; (b) transferring the equilibrium mixture to a larger reaction vessel; (c) adding a small amount of LiOH(s), which reacts with HCl to give LiCl(s) and H2O(l).

Explanation / Answer

a. increasing the temperature causes the net reaction to go from left to right. This always occurs in an endothermic reaction. Increasing the temperature will have no effect on the partial pressure of NH3 so it will stay the same. b. Increasing the volume will cause it to move to the side with most # of moles of gas molecules. This is the right side so it will shift from left to right. Increase in volume will cause an increase in the partial pressure of NH3 c. Adding LiOh to react with HCl means you are using up HCl which causes the reaction to go from right to left. There is no effect on the pressure so the partial pressure of NH3 will remain the same Hope this helped

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