Solid carbon can form either carbon monoxide or carbon dioxide when burned

CHEMISTRY · Single correct · A Level · Chemistry · Energetics · Energetics

Problem

Solid carbon can form either carbon monoxide or carbon dioxide when burned, depending on the amount of oxygen available: (1) C(s)+O2(g)→CO2(g)ΔH=−394 kJ\text{C}(s)+\text{O}_2(g)\rightarrow\text{CO}_2(g)\quad\Delta H=-394\,\text{kJ} (2) 2 C(s)+O2(g)→2 CO(g)ΔH=−221 kJ2\,\text{C}(s)+\text{O}_2(g)\rightarrow 2\,\text{CO}(g)\quad\Delta H=-221\,\text{kJ} A sample containing 1.00 mol1.00\,\text{mol} of C is reacted with 0.60 mol0.60\,\text{mol} of O2\text{O}_2 at constant pressure, and the reaction proceeds until either carbon or oxygen is completely consumed with no solid carbon remaining. Which of the following values is closest to the heat released? (a) +1.1×102 kJ+1.1\times10^{2}\,\text{kJ} (b) −1.7×102 kJ-1.7\times10^{2}\,\text{kJ} (c) −1.1×102 kJ-1.1\times10^{2}\,\text{kJ} (d) −2.2×102 kJ-2.2\times10^{2}\,\text{kJ}

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