A chemist measures the energy change DeltaH during the following reaction: 2NH3(

Question

A chemist measures the energy change DeltaH during the following reaction:


2NH3(g) --> N2(g) + 3H2(g) DeltaH = 160. kJ



A) Is the reaction ENDOthermic or EXOthermic?

I chose ENDO, but I don't know if I'm correct.

B) Suppose 54.3g of NH3 react.
Will any heat be released or absorbed? I chose Released but again, I'm not sure.
The options are
a) Yes, absorbed
b) Yes, released
c) No

C) If you said heat WILL be released or absorbed in the second part of this question, calculate HOW MUCH heat will be released or absorbed. Round to three sig figs.

Explanation / Answer

A.      As DeltaH for the reaction is +ve heat is absorbed in the reaction. Hence it is endothermic reaction.

B.      As reaction is endothermic heat will be absorbed.

C.      Moles of NH3 reacted=54.3/17=3.194mol

Heat of reaction=160/2=80kJ/mol

Heat absorbed=80*3.194=255.53 kJ

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