Question

Consider the reaction C12H22O11 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H2O (l) in which 10.5 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/oC (including its water). The temperature inside the calorimeter was found to increase by 20.2 oC. Based on this information, what is the heat of this reaction per mole of sucrose?

Answer 1

The heat of reaction is 4938 kJ/mole

Step-by-step explanation:

It is possible to calculate the heat of a reaction using:

`q = SpecificHeat *dT`

For the reaction:

C₁₂H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l)

Specific heat: 7,50kJ/°C

dT = 20,2°C

Thus, q = 151,5 kJ

The moles of sucrose are: 10,5g /342,2965 g/mol = 0,030675 moles

The heat of reacton is:

`(151,5 kJ)/(0,030675moles) = 4938 kJ/mol`

I hope it helps!