Given the following reactions N₂ (g)+ O₂ (g)→ 2NO (g)ΔH = +180.7 kJ 2NO( g)+ O₂ (g)→ 2NO₂ (g)ΔH = -113.1 kJ The enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO₂ (g)→ N₂ (g)+ 2O₂ (g) Is ________ kJ. A)67.6 B)-67.6 C)293.8 D)-293.8 E)45.5

Question

Quizplus · Accepted Answer

Using Hess's Law, we can add the first and second reactions and reverse the second reaction to cancel out the oxygen sulfide (O2S) and nitrogen oxide (NO) intermediates to get the net equation for the decomposition of nitrogen dioxide: N₂ (g) + 2NO(g) → N₂(g) + O2(g) + N2(g) We add the enthalpies of the reactions to get the enthalpy for the net equation: ΔH = (+180.7 kJ) + (-113.1 kJ) = +67.6 kJ Therefore, the answer is B) -67.6 kJ.

Given the Following Reactions N2 (G)+ O2 (G)→ 2NO (G)ΔH

Given the Following Reactions N₂ (G)+ O₂ (G)→ 2NO (G)ΔH