Butane (C₄H₁₀)undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water.Given $\Delta$H°_f[C₄H₁₀(g)] = -124.7 kJ/mol, $\Delta$H°_f[CO₂(g)] = -393.5 kJ/mol, $\Delta$H°_f[H₂O(g)] = -241.8 kJ/mol, how much energy is released (kJ)when 8.30 g of butane is burned? A)22,100 kJ B)2,658.3 kJ C)379 kJ D)759 kJ E)2,910 kJ

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The Answer of Butane (C₄H₁₀)undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water.Given $\Delta$H°_f[C₄H₁₀(g)] = -124.7 kJ/mol, $\Delta$H°_f[CO₂(g)] = -393.5 kJ/mol, $\Delta$H°_f[H₂O(g)] = -241.8 kJ/mol, how much energy is released (kJ)when 8.30 g of butane is burned? A)22,100 kJ B)2,658.3 kJ C)379 kJ D)759 kJ E)2,910 kJ

Butane (C4H10)undergoes Combustion in Excess Oxygen to Generate Gaseous Carbon Δ\DeltaΔ

Butane (C₄H₁₀)undergoes Combustion in Excess Oxygen to Generate Gaseous Carbon $\Delta$