A 100.-gram sample of H2O () at 22.0°C absorbs 8360 joules of heat. What will be the final temperature of the water?

Question

Kamila Koch

Chemistry

9 June, 01:58

A 100.-gram sample of H2O () at 22.0°C absorbs 8360 joules of heat. What will be the final temperature of the water?

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Jocelynn Ball · Answer 1

In this problem you need to use the equation q=mcΔT. q is the amount of heat absorbed or released, m is the mass of what ever the q value is referring to, delta T is the temperature change, and c is the specific heat capacity of what ever q is referring to. With that equation you can rewrite it as T (final) = (q/mc) + T (intital). In the question that you gave, m=100g, T (initial) = 22.0°C, q=8360J, and c=4.179J/g°C. when you plug everything in T (final) should equal 41.9°C.