A student is asked to determine what mass of butane, , needs to burn in order to raise the temperatu — Thermodynamics Chemistry Question

$q = mc\Delta T$
$q = (1650\text{ g})(0.810\text{ J}/(\text{g}\cdot^\circ\text{C}))(180.^\circ\text{C}) = 241,000\text{ J} = 241\text{ kJ}$

1 point is earned for the correct calculation of the energy.

$225.26\text{ g} - 218.20\text{ g} = 7.06\text{ g butane}$
$7.06\text{ g} \times \frac{1\text{ mol}}{58.12\text{ g butane}} = 0.121\text{ mol butane}$

1 point is earned for the correct calculation of the number of moles with the correct number of significant figures.

$0.121\text{ mol butane} \times \frac{2659\text{ kJ produced}}{1\text{ mol butane}} = 322\text{ kJ}$

1 point is earned for the correct determination of the amount of heat produced.

Yes, the answers to parts (a) and (c) support the hypothesis. The amount of heat generated from the combustion of the butane is greater than the amount of heat required to cause the temperature change of the sand, indicating that some of the heat from the combustion of butane was lost.

1 point is earned for a correct choice and a valid explanation.