Ask Question
19 September, 22:15

How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.ΔHvap = 40.7 kJ/molCliq = 4.18 J/g°CCgas = 2.01 J/g°CCsol = 2.09 J/g°CTmelting = 0°CTboiling = 100°C

+4
Answers (1)
  1. 19 September, 22:32
    0
    energy required=qnet=87.75kJ

    Explanation:

    we will do it in three seperate step and then add up those value.

    first step is to heat the sample of water upto 100C i. e upto boiling pont. because just after this sample of water started vaporization.

    q 1 = m c (T2-T1)

    q1 = 36.0 g (4.18 J/gC) (100 - 65 C)

    q1 = 5267 J = 5.267kJ

    next is to vaporize the sample at 100C

    q2 = 36.0 g / 18.0 g/mol X 40.7 kJ/mol

    q2 = 81.4 kJ

    Finally, heat the steam upto 115C

    q3 = m c (T2-T1)

    q 3 = 36.0 g (2.01 J/gC) (115-100C)

    q3 = 1085 J = 1.085kJ

    qnet=q1 + q2 + q3

    energy required=qnet=87.75kJ
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.ΔHvap = ...” in 📗 Chemistry 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