Calculating the Heat of Reaction from the Stoichiometry How much heat is evolved when [latex]9.07 × 10^5[/latex] g of ammonia is produced according to the following equation? (Assume that the reaction occurs at constant pressure.) [latex]N_2(g) + 3H_2(g) → 2NH_3(g); ΔH = -91.8 kJ[/latex] PROBLEM STRATEGY The calculation involves converting grams of [latex]NH_3[/latex] to moles of [latex]NH_3[/latex] and then to kilojoules of heat. Grams of [latex]NH_3[/latex] → moles of [latex]NH_3[/latex] → kilojoules of heat You obtain the conversion factor for the second step from the thermochemical equation, which says that the production of 2 mol [latex]NH_3[/latex] is accompanied by [latex]q_p[/latex] = -91.8 kJ.

[latex]9.07 \times 10^5 \cancel{g NH _3} \times \frac{1 \cancel{mol NH _3}}{17.0 \cancel{g NH _3}} \times \frac{-91.8 kJ }{2 \cancel{mol NH _3}} = -2.45 \times 10^6 kJ [/latex] Thus, [latex]2.45 \times 10^6 kJ \text { of heat evolves. }[/latex]

Question 6.4: Calculating the Heat of Reaction from the Stoichiometry How ...

General Chemistry

Calculating the Heat of Reaction from the Stoichiometry

How much heat is evolved when $9.07 \times 10^5$ g of ammonia is produced according to the following equation? (Assume that the reaction occurs at constant pressure.)

N_2(g) + 3H_2(g) \to 2NH_3(g); ΔH = -91.8 kJ

PROBLEM STRATEGY

The calculation involves converting grams of $NH_3$ to moles of $NH_3$ and then to kilojoules of heat.

Grams of $NH_3$ → moles of $NH_3$ → kilojoules of heat

You obtain the conversion factor for the second step from the thermochemical equation, which says that the production of 2 mol $NH_3$ is accompanied by $q_p$ = -91.8 kJ.

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