How much heat is produced if 7.0 moles of butane combust completely?

To determine the amount of heat produced during the complete combustion of butane, one can start by looking at the balanced chemical equation for the combustion of butane (C4H10):

[ \text{C}4\text{H}{10} + 13/2 \text{O}_2 \rightarrow 4 \text{CO}_2 + 5 \text{H}_2\text{O} ]

In this reaction, butane combusts in the presence of oxygen to produce carbon dioxide and water. The enthalpy of combustion (ΔH_comb) for butane is known to be approximately -2850 kJ per mole of butane combusted. This value signifies that 2850 kJ of heat is released when one mole of butane undergoes complete combustion.

To find the total heat produced by 7.0 moles of butane, one would multiply the heat released per mole by the number of moles combusted:

[ \text{Total heat} = \text{moles of butane} \times \Delta H_{\text{comb}} ] [ = 7.0 , \text{mol} \times -2850 , \