Octane, C_8 H_18, burns according to the balanced equation: 2 C_8 H_18 (l) + 25

Question

Octane, C_8 H_18, burns according to the balanced equation: 2 C_8 H_18 (l) + 25 O_2 (g) rightarrow 16 CO_2 (g) + 18 H_2 O (l) Delta H_rxn = -10,920 KJ/mol If an engine burns 277 moles of C_8 H_18. What is the heat, q_rxn, associated with this reaction? -39,42 kJ -78.85 kJ -1,510,000 kJ -3,030,000 kJ -6,050,000 kJ What is the value of Delta H degree_rxn for the reaction 2 KCl(s) + 3 O_2 (g) rightarrow 2 KCIO_3 (s)? Delta H degree f for KCIO_3 (s) is -391.20 kJ/mol Delta H degree_f for KCI (s) is -435.87 kJ/mol + 89.34 kJ/mol -89.34 kJ/mol -1654.14 kJ/mol -62.67 kJ/mol -827.02 kJ/mol

Explanation / Answer

The answer is the D because the Hrxn is -10920kJ/mol of Octane, therefore:

q=-10920*277 = -302484 kJ

Regards.

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