How many grams of water would require #2.20 * 10^4# calories of heat to raise its temperature from #34.0°C# to #100.0°C#?
333.33 g of water.
The relationship between energy in short calories (E), mass in grams (m), temperature change (d), and specific heat in cal/g (C) is: E = m. C.d
We know the energy value, which is 22,000 cal, the specific heat capacity of water is 1 cal/g, and the temperature change is 66 degrees celcius.
So rearranging for m, we have m = E (C..d) which is 22000 / (1 x 66) = 333.33 g of water.