How much heat is produced by burning 4.00 moles of acetylene under standard state conditions?

Combustion of acetylene is represented as:

C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(l)

ΔHrxn = ∑nΔH°f(products) - ∑nΔH°f(reactants)

n = # moles

ΔH°f = standard enthalpy of formation from thermochemical tables

ΔHrxn = [2ΔH°f(CO2)+ΔH°f(H2O)] - [ΔH°f(C2H2)+ 3/2ΔH°f(O2)]

          = [2(-393.5)-285.8] - [226.7 + 0] = -1299.5 kJ/mol

Based on the above:

1 mole of acetylene produces -1299.5 kJ of heat

Therefore, heat produced by burning 4 moles is= -1299.5 *4 = -5198 kJ

Ans: -5198 kJ of heat is produced by burning 4.00 moles of acetylene under standard state conditions

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

i think it's c. i'm not sure but i think so.