Determine $\Delta$G_rxn for C₄H₁₀( ) + O₂(g) $\rightleftarrows$ 4CO₂(g) + 5H₂O(g) given the following. Substance $\Delta$G (J/mol · K) C₄H₁₀( ) -15)0 CO₂(g) -394.4 H₂O(g) -228.57

Question

Quizplus · Accepted Answer

First, we need to write out the balanced chemical equation for the reaction:

11eaae02_08a4_63a8_95d8_2df823a85b0d_TB3833_11 + 11eaae02_08a4_8ab9_95d8_b76c374d308e_TB3833_11 → 3F1F1F1S1F1F1F10G + 4CO + 5H2O

Now we can use the standard enthalpy of formation values to calculate the enthalpy of the reaction:

ΔH°f(CO) = -110.5 kJ/mol 
ΔH°f(H2O) = -241.8 kJ/mol

ΔH°rxn = ∑ΔH°f(products) - ∑ΔH°f(reactants) 
ΔH°rxn = (3 mol)(0 kJ/mol) + (4 mol)(-110.5 kJ/mol) + (5 mol)(-241.8 kJ/mol) - [(1 mol)(-2705 kJ/mol) + (1 mol)(-608.0 kJ/mol) + (11 mol)(-1791 kJ/mol)] 
ΔH°rxn = -2705 kJ/mol

Therefore, the answer is A: -2705 kJ/mol.

Determine Δ\DeltaΔ Grxn for C4H10( ) + O2(g) ⇄\rightleftarrows⇄ 4CO2(g) + 5H2O(g) Given the Following

Determine $\Delta$ G_rxn for C₄H₁₀( ) + O₂(g) $\rightleftarrows$ 4CO₂(g) + 5H₂O(g) Given the Following