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Chemistry

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When 23.6 of calcium chloirde CaCl2 was dissolved in water in a calorimeter, the temperature rose from 25.0 degrees C to 21.56 degrees C. If the heat capacity of the solution and the calorimeter is 1071 J/ degrees C, what is the enthalpy change when 1 mol of sodium nitrate dissolves in water? The solution process is

NaNO3 + Na + NO3
Delta H = ?

  • Chemistry - ,

    You need to re-read the problem you posted. First, you say the temperature rose but going from 25.0 to 21.56 is not rising. Second, you provide data for CaCl2 but you ask for answers for NaNO3. If this is part of a lab (or a question from a multipart question), there needs to be more data. Something is missing.

  • Chemistry - ,

    sorry it is supposed to say
    When 23.6 of calcium chloirde CaCl2 was dissolved in water in a calorimeter, the temperature rose from 25.0 degrees C to 38.7 degrees C. If the heat capacity of the solution and the calorimeter is 1258 J/ degrees C, what is the enthalpy change when 1 mol of sodium nitrate dissolves in water? The solution process is

    CaCl2 ----> Ca2+ + 2Cl
    Delta H=?

    Sorry I read the wrong question my fault I appoligize

  • Chemistry - ,

    I can GUESS that the 23.6 is GRAMS and not mols. I can also GUESS that the next to last sentence should read "when 1 mol calcium chloride dissolves in water?" If my guesses are correct, then
    q = heat evolved on solution = Cp x delta T.
    q = 1258 J/oC x delta T for 23.6 g CaCl2.
    Therefore, you know q (delta H) for 23.6 g CaCl2. You want to know the q for 1 mol CaCl2 or 111 g CaCl2. A proportion. You need to obtain the exact molar mass of CaCl2 since I used round numbers. I just estimated it.

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