Ask Question
24 June, 21:33

How much heat is required to warm 1.20 l of water from 26.0 ∘c to 100.0 ∘c? (assume a density of 1.0g/ml for the water.) ?

+2
Answers (1)
  1. 24 June, 21:40
    0
    When we have the volume = 1.2 L

    and density = 1000 g/L

    ∴ mass of water (m) = volume * density

    = 1.2 * 1000

    = 1200 g

    according to this formula, we can get the amount of Heat q:

    q = m * C * ΔT

    = 1200 g * 4.18 * (100 - 26)

    = 371184 J
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “How much heat is required to warm 1.20 l of water from 26.0 ∘c to 100.0 ∘c? (assume a density of 1.0g/ml for the water.) ? ...” 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