Question

Which one of the following reactions would produce the largest amount of heat
per mole of hydrogen?
A) C(s) + 2 H2 (g) CH4 (g) AH° = -74.9
kJ/mol
B) N2O (g) + 3 H2 (g) N2H4 (g)+ H2O (l)
AH° = -316.8 kJ/mol
C) 2 H2(g) + O2 (g) 2 H2O (l) AH° = -571.6
kJ/mol
D) N2 (g) + 3 H2 (g) 2 NH3 (g) AH° = -91.8
kJ/mol

Answer 1

Answer:

C) 2 H2(g) + O2 (g) 2 H2O (l) AH° = -571.6

kJ/mol

Explanation:

The magnitude of heat released in an exothermic reaction is shown by the magnitude of the change in enthalpy.

The more negative the enthalpy change of the reaction, the more the heat released by the process.

Hence,  2 H2(g) + O2 (g) 2 H2O (l) AH° = -571.6 kJ/mol has the most negative value of enthalpy change hence the greatest amount of heat is released in this reaction.

Answer 2

The reaction which would produce the largest amount of heat per mole of hydrogen is; Choice C: 2H2(g) + O2 (g). ===> 2 H2O (l) AH° = -571.6

AH° = -571.6kJ/mol.

According to the question;

• We are required to identify the reaction which would produce the largest amount of heat per mole of hydrogen.

It is evident that all the reactions are exothermic; the reactions release heat.

• In essence, the reaction which produces the largest amount of heat is that with the largest negative enthalpy change, AH.

In this scenario; the reaction that would produce the largest amount of heat per mole of hydrogen is Choice C: 2H2(g) + O2 (g) =====> 2 H2O (l) AH° = -571.6 kJ/mol

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