Consider 324 g of water in the liquid state the system at an

Consider 32.4 g of water in the liquid state (the system) at an initial temperature of 32.5o C and at atmospheric pressure (1.00 atm). Assume that the heat exchanged between the system and its surroundings is q = - 425 J and the heat capacity of water liquid is 1.00 cal/g.K. What is the final temperature in K of the water?

Solution

Heat capacity is defines as the amount of energy required to raise the temperature by 1 deg.

Here the heat capacity of water = 1 cal/g-K

Given heat energy is Q = 425 J = 425*0.239 = 101.580 cal

Heat energy required to raise the temperature of 32.4 gms is

H = 32.4 cal

Now the raise in temperature

dT = 101.580/32.4 = 3.14

Now the final temperature Tf = 32.5+3.14 = 35.64 deg C