Question

The nutrition label tells us that 13 g of a serving of gummy bears (i.e. 10 gummy bears) is made of sugars. Let's assume that all of the sugar is sucrose. The balanced reaction for the combustion of sucrose is given below. How much heat is released from the combustion of the sucrose in a single gummy bear?
2C12H22O11+24O2→24CO2+22H2O ΔHrxn=−11,286kJ

Answer 1

This problem is providing the mass of gummy bears which are assumed to contain 13 g of sucrose, which undergoes combustion and produces -214.3kJ of heat according to the following:

Heat of reaction

In chemistry, when a fuel undergoes combustion, a reaction with oxygen, it produces carbon dioxide and water in a complete combustion. In such a way, with the given reaction, we can write the heat of reaction as -11,286 kJ per mole of reaction:

$\Delta H=-11,286\frac{kJ}{mol\ rxn}$

Which means that if we need the total heat released by 13 g of sucrose, one must apply the following dimensional analysis including this fuel's molar mass (342.3 g/mol):

$Q=-11,286\frac{kJ}{mol\ rxn}*\frac{1mol\ rxn}{2molC_1_2H_2_2O_1_1}*13gC_1_2H_2_2O_1_1 *\frac{1molC_1_2H_2_2O_1_1}{342.3gC_1_2H_2_2O_1_1} \\\\Q=-214.3kJ$

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