Question

Consider the reaction C12H22O11(s) +12O2(g) --->12CO2(g)+11H2O(l)

in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/C. The temperature increase inside the calorimeter was found to be 22.0 C. Calculate the change in internal energy, delta E, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to four significant figures.

DeltaE = ? kj/mol

Answer 1

The change in internal energy per mole of sucrose is 5651 kJ/mol

Step-by-step explanation:

For the reaction:

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

The heat generated is:

q = CΔT

Where q is the heat generated, C is heat capacity (7,50 kJ/°C) And ΔT is change in temperature (22,0°C)

Replacing:

q = 165 kJ

This heat is produced by:

10,0g sucrose × (1 mol / 342,2965g) = 0,0292 moles.

Thus, the change in internal energy per mole of sucrose is:

165kJ / 0,0292mol = 5651 kJ/mol

I hope it helps!