For the reaction
MnO₂(s) + CO(g) $\rightarrow$ MnO(s) + CO₂(g) $\Delta$ H = -151 kJ/ mol_rxn.
How many moles of MnO₂ are required in order for 418 kJ of heat to be released?

Name: For the reaction MnO 2 (s) + CO(g) $\rightarrow$ MnO(s) + CO 2 (g) $\Delta$ H = -151 kJ/ mol rxn . How many moles of MnO 2 are required in order for 418 kJ of heat to be released?
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Question

For the reaction MnO₂(s) + CO(g) $\rightarrow$ MnO(s) + CO₂(g) $\Delta$ H = -151 kJ/ mol_rxn. How many moles of MnO₂ are required in order for 418 kJ of heat to be released?

Quizplus · Accepted Answer

The reaction releases 151 kJ per mole of MnO2. To release 418 kJ, divide 418 kJ by 151 kJ/mol, which equals approximately 2.77 moles.

For the Reaction MnO2(s) + CO(g) →\rightarrow→ MnO(s) + CO2(g) Δ\DeltaΔ H = -151 KJ/ Molrxn

For the Reaction
MnO₂(s) + CO(g) $\rightarrow$ MnO(s) + CO₂(g) $\Delta$ H = -151 KJ/ Mol_rxn