The combustion of 1.00 mol of glucose, C6H12O6, releases 2820 kJ of heat. If 2.0 g of glucose is burned in a calorimeter containing 1.0 kg of water, and the temperature increases by 3.5 oC, what is the heat capacity of the calorimeter?

The heat capacity of the calorimeter is 4.76 kJ/°C

Explanation:

Step 1: Data given

1.00 mol of glucose releases 2820 kJ of heat

Mass of glucose = 2.0 grams

Mass of water = 1000 grams

The temperature increases with 3.5 °C

Step 2: Calculate moles

moles glucose = mass glucose / molar mass glucose

moles glucose = 2.0 grams / 180.16 g/mol

moles glucose = 0.0111 moles

Step 3: Calculate heat produced by the combustion

Heat produced = 2820 kJ/mol * 0.0111 moles

Heat produced = 31.302 kJ = 31302 J

Step 4: Calculate heat absorbed by the water

Q = m*c*ΔT

⇒ with m = the mass of water = 1000 grams

⇒ with c = the specific heat of water = 4.184 J/g°C

⇒ with ΔT = The change in temperature = 3.5 °C

Q = 1000 * 4.184 * 3.5

Q = 14644 J absorbed by the water

Step 5: Calculate heat basorbed by the calorimeter

Q = 31302 - 14644 = 16658 J absorbed by the calorimeter

Step 6: Calculate the heat capacity of the calorimeter

c = 16658 J / 3.5 °C

c = 4759 J/°C = 4.76 kJ/°C

The heat capacity of the calorimeter is 4.76 kJ/°C