What is δe in kj for a system that receives 1.79 kj of heat from surroundings and has 4.51 kcal of work done on it at the same time. 1 cal = 4.184 j.

20.7 kJ

Explanation:

According to first law of thermodynamics:

=Change in internal energy

q = heat absorbed or released

w = work done or by the system

w = work done on the system=  {Work is done on the system is positive as the final volume is lesser than initial volume}

w = 4.51 kcal =    (1kcal = 4.184kJ)

q = +1.79 kJ   {Heat absorbed by the system is positive}

Thus for a system that receives 1.79 kJ of heat from surroundings and has 4.51 kcal of work done on it at the same time is 20.7 kJ

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