Question

1.10 g of glucose was completely burnt in a copper calorimeter. The temperature of the water
increased from 25.85 °C to 36.50 °C.

Calculate the enthalpy of combustion of glucose from the data below. Assuming the heat released by combustion reaction is absorbed by both water and copper calorimeter.

Mass of water/g 200.00
Specific heat capacity of water: 4.18
Mass of copper/g 120.00
Specific heat capacity of copper/g-1K-1

Answer 1

You didn't write in the heat capacity of the calorimete
q = [mass H2O x specific heat H2O x (delta T)] + [Ccal x (delta T)
q = [200 x 4.18 x (36.50-25.85)] + Ccal x (36.50-25.85)] = ?
That is q for 1.10 g. You don't say but most problems like this want enthalpy of combustion per mol. To convert to kJ/mol do this.
q from above x 180 g/1.10 g = ? in J/mol and usually these are convert to kJ/mol. Finally the heat of combustion is the negative of q. q is the heat absorbed by the calorimeter but the combustion gives off heat so it is negative.