During the calculation process, how must the following reaction and its ΔH°rxn be manipulated? N2(g) + O2(g) → 2 NO(g) ΔH°rxn = +183 kJ A) the reaction must be doubled and its ΔH°rxn must be doubled B) the reaction must be doubled and its ΔH°rxn must undergo a sign change C) the reaction must be quadrupled and its ΔH°rxn must be quadrupled and undergo a sign change
The standard reaction enthalpies given below are used to determine ΔH°rxn for the following reaction:
4 NO(g) + 2 O2(g) → 4 NO2(g) ΔH°rxn = ?
Given:
N2(g) + O2(g) → 2 NO(g) ΔH°rxn = +183 kJ
1/2 N2(g) + O2(g) → NO2(g) ΔH°rxn = +33 kJ
During the calculation process, how must the following reaction and its ΔH°rxn be manipulated?
N2(g) + O2(g) → 2 NO(g) ΔH°rxn = +183 kJ
A) the reaction must be doubled and its ΔH°rxn must be doubled
B) the reaction must be doubled and its ΔH°rxn must undergo a sign change
C) the reaction must be quadrupled and its ΔH°rxn must be quadrupled and undergo a sign change
D) the reaction must be halved and its ΔH°rxn must also be halved
E) the reaction must be doubled and its ΔH°rxn must be doubled and undergo a sign change
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