Question

What would be the final temperature if `3.31 * 10^3` joules of heat were added to 18.5 grams of water at 22.0°C?

Answer 1

I found: `T_f=64.6^@C`

Explanation:

We can try using the general relationship between heat `Q` (lost or gained) and change in temperature `DeltaT` of a mass `m` of a substance of specific heat `c` (in our case water: `c_("water")=4.2J/(g^@C)`):

`Q=mcDeltaT`

with our data:
`3.31xx10^3=18.5*4.2*(T_f-22)`
rearranging we get:
`T_f=64.6^@C`