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If all the energy obtained from burning 1.23 pounds of propane (fuel value is 11.09 kcal/g) is used to heat 125.0 kg of water at an initial temperature of 21.8 °C, what is the final temperature?

The heat, q, released by burning propane is absorbed by the water. Use the following formula to find the temperature change, ÄT,
q = m*c*(Change in temperature)
Where m is mass and c is specific heat

I've done it several different ways and I keep getting 21.8 for an answer and it says that is wrong.

  • chemistry -

    Change 1.23 pounds to grams.
    1.23 pounds x (453.6 g/lb) = ?
    ?g x 11,090 cal/g = calories of heat produced = y
    y = mass H2O x specific heat H2O x (Tfinal-Tinitial).
    I would use 125,000 for mass H2O. I get something like 70 C. You know it can't be 21.8. That's the starting temperature and you're adding bunches of heat. T must go up.

  • chemistry -


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