Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing

morganfrank

  • 2 years ago

At 1 atm, how much energy is required to heat 93.0 g of H2O(s) at –24.0 °C to H2O(g) at 115.0 °C?

  • This Question is Open
  1. aaronq
    • 2 years ago
    Best Response
    You've already chosen the best response.
    Medals 2

    you need to use 2 equations, in 5 steps. (1) \(q=H_{fusion/vap}*m\) (2) \(q=m*C_p*\Delta T\) |dw:1382470856637:dw| In A, your heating up the ice from -24 to 0 degrees: use equation (2) and the appropriate \(C_P\). In B, the ice is melting, use equation (1), use appropriate \(H_{fusion}\) In C, you're heating up the water form 0 to 100 degrees, use equation (2). Use appropriate \(C_p\). In D, you're vaporizing/boiling the water, use equation (1), use appropriate \(H_{vap}\). In E, you're heating up the water vapour/steam, use equation (2), use appropriate \(C_p\).

  2. Not the answer you are looking for?
    Search for more explanations.

    • Attachments:

Ask your own question

Sign Up
Find more explanations on OpenStudy
Privacy Policy