I tried but I can't help me please?

Burning 0.510 g of ethanol resulted in a 10.00 ∘C rise in the temperature of the 200.0 mL of water in the calorimeter. Assume that the calorimeter is not perfect.

1-How much energy was released by burning 0.510 g of ethanol?

2-How much energy is required to raise the temperature of 200.0 mL of water by 10.00 ∘C?

3, A: How much energy was lost to the surroundings in this calorimetric experiment? Express this value as a total number of kilojoules as well as a percentage of the total heat released by burning ethanol.

kilojoules of energy loss =

percentage of energy loss =

4-What is the heat capacity of this calorimetric apparatus (𝐶cal)?

2 Answers

  • 7 months ago


    The source below says the heat of combustion for liquid ethanol is 29666 kJ/kg, so:

    (0.000510 kg ethanol) x (29666 kJ/kg ethanol) = 15.12966 kJ = 15.1 kJ produced


    (4.184 J/g·°C) x (200.0 g) x (10.00°C) = 8368 J


    (15.12966 kJ) - (8.368 kJ) = 6.762 kJ = 6.76 kJ lost

    (6.762 kJ) / (15.12966 kJ) = 0.44693 = 44.7% of the total was lost


    Supposing all the energy "lost" ended up in the calorimeter, and supposing the temperature change of the calorimeter was the same as the water, and supposing this question about the "calorimetric apparatus" is asking about the 𝐶cal of the calorimeter alone, excluding its water.

    (6.762 kJ) / (10.00°C) = 0.676 kJ/°C = 676 J/°C

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  • Anonymous
    7 months ago

    Its very simple. I will give you the answer, but you first have to choose my answer as best then I will edit it an put the full answer. 

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