## Answers

According to the first law of thermodynamics, the change in internal energy (E) is the sum of heat (q) and work (w):

E = q + w

Since heat is absorbed by the system from the surroundings, heat (q) is positive; also, work (w) is positive since work is done on the system.

Converting the values of heat to work to Joules, we get:

q = 0.297 kJ 10^{3} J 1 kJ [1 kJ = 10^{3} J]

= 297 J

w = 0.750 kcal 10^{3}cal 1 kcal 4.184J 1 cal [1 kcal = 10^{3}cal ; 1 cal = 4.184 J]

= 3138 J

Therefore, E_{int} = q + w = +297 J - [-3138 J] = 3435 J

There is an increase in internal energy.

3435 J can be written as :

**Change in internal energy = 3.435 10 ^{3} J**

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