A Constant Volume Calorimeter's Temperature Increases by 2 $\Delta$ T)
A) 5623 KJ/mol
B) 5640 KJ/mol
C) 8,434 KJ/mol

A constant volume calorimeter's temperature increases by 2.34 K when a standard compound is combusted, releasing 2.14 kJ of energy. A 0.5623 g sample of sucrose, C₁₂H₂₂O₁₁, is then combusted in the same calorimeter and a temperature increase of 10.13 K is noted. What is the energy released per mole of sucrose combusted?(C = 75.291 J/mol . K for H₂O; q = C_cal $\Delta$ T)

A) 5623 kJ/mol
B) 5640 kJ/mol
C) 8,434 kJ/mol
D) 10,355 kJ/mol
E) 3168 kJ/mol