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

To determine the amount of heat produced by burning 4.00 moles of acetylene under standard state conditions, we can use the balanced chemical equation for the combustion of acetylene:

2 C2H2 + 5 O2 -> 4 CO2 + 2 H2O

From the balanced equation, we can see that 2 moles of acetylene (C2H2) react to produce 4 moles of carbon dioxide (CO2) and 2 moles of water (H2O).

The standard enthalpy change (∆H°) for the combustion of acetylene is -1299 kJ/mol. This means that for every mole of acetylene burned, 1299 kJ of heat is released.

To calculate the amount of heat produced by burning 4.00 moles of acetylene, we can use the following equation:

Heat produced = moles of acetylene * ∆H°

Heat produced = 4.00 moles * -1299 kJ/mol

Heat produced = -5196 kJ

Therefore, 4.00 moles of acetylene burned under standard state conditions would produce -5196 kJ of heat.