I need help with this question! I have looked at other posts & try doing their m
ID: 539790 • Letter: I
Question
I need help with this question! I have looked at other posts & try doing their methods, and it still ends up wrong.
Question 26 0.2 pts Consider the reaction C12H22011 (s) + 12 02 (g) 12 CO2 (g) + 11 H2O (1) in which 10.0 g of sucrose, C12H22011, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/oC. The temperature increase inside the calorimeter was found to be 22.0 °C. What is the heat of this reaction per mole of sucrose? Enter your answer numerically, in terms of kJ/mol and to three significant figures. Be sure to note if this reaction is exothermic or endothermic.Explanation / Answer
Mass of sucrose = 10.0 g ,
Molar mass of sucrose = 342.3 g/mol
Number of moles of sucrose = 10.0 g/ 342.3 g/mol = 0.0292 mole
We know
Q = C T
Where, Q = heat of a reaction, C = heat capacity, T= Temperure change
Q = (7.50 KJ/oC)*22 oC = 165 KJ
Heat of reaction per mole = 165 KJ/0.0292 mol
= 5650.685 KJ/mol
Since heat will released during combustion reaction, hence heat of reaction will be in negative sign
Heat of reaction = -5650.685 KJ/mol