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, ΔE, for this reaction per mole of sucrose.

-5648kj/mol

Explanation:

The mass of C12H22011 is 10g

Its molar mass is 342.2965g/mol

Q = -Ccal∆T

= 7.50(22⁰c)

= -165.0kj

To get the internal energy

= -165.0kj/10g x 342.2965/1

= -56478.9225/10

= -5648kj/mol

In conclusion, -5648kj/mol is the change in internal energy, ΔE, for this reaction per mole of sucrose.

Another way to get this answer is;

10/342.2965

= 0.02921

-165.0kj / 0.02921

= -5648kj/mol

stupid i wont let you get a chance

explanation:

a electronegativity decreases beacuse the size of nucleus is bigger.