Ask Question
5 June, 02:26

Suppose you want to heat a 600 mL cup of water in the microwave from 20° to 100°C. Water has a specific heat capacity of 4.184 J/g°C and a density of 1.00 g/mL in this temperature range. How much energy is required to heat the cup of water?

+2
Answers (1)
  1. 5 June, 02:44
    0
    The quantity of heat required to to heat the cup of water through a temperature change of 80°C = 200.83 kJ

    Explanation:

    Density = mass/Volume.

    ∴ mass = Density * volume

    Where Density of water = 1.00 g/mL, volume of water = 600 mL

    Mass = 1 * 600 = 600 g.

    (Q) = cm (ΔT) ... equation 1

    Where Q = quantity of heat, c = specific heat capacity of water, m = mass of water, ΔT = T₁-T₂ = change in temperature.

    Where c = 4.184 J/g°C, m = 600 g, ΔT = T₁-T₂ = 100 - 20 = 80°C

    Substituting these values into equation 1,

    Q = 4.184 * 600 * 80

    Q = 200832 J = 200.83 kJ

    Therefore the quantity of heat required to to heat the cup of water through a temperature change of 80°C = 200.83 kJ
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Suppose you want to heat a 600 mL cup of water in the microwave from 20° to 100°C. Water has a specific heat capacity of 4.184 J/g°C and a ...” in 📗 Physics if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers