A closed 2.0-L container holds 3.0 mol of an ideal gas. If 200 J of heat is adde

Question

A closed 2.0-L container holds 3.0 mol of an ideal gas. If 200 J of heat is added. what is the change in internal energy of the system? zero 100 J 150 J 200J A 4-mol ideal gas system undergoes an adiabatic process where it expands and does 20 J of work on its environment. What is its change in internal energy? -20 J -5 J zero +20J A gas is taken through the cycle shown in the pV diagram in the figure. During one cycle, how much work is done by the gas? As ideal Cannot heat engine has an efficiency of 0.600. If it operates between a deep take with a constant temperature of 294.0k and a hot reservoir ,what is the temperature of the hot reservoir 735K 490K 470K 784K

Explanation / Answer

15) By first law of thermodynamics,
Heat given given to a system = Work done by the system + Increase in internal energy.

Here, the gas is enclosed in a closed container, so there is no change in volume, no work is done by gas.
All the heat given is utilized to increase the internal energy.
So, the change in internal energy is same as heat given to system, which is 200 J
option D is the right answer.

16) Under adiabatic process, no heat exchange takes place.
so work done by the system results in decrease of internal energy.
Change in internal energy = negative of work done = -20 J
option A is the right answer.

17) Work done by the system = Area enclosed in the cycle = P0*3V0 = 3P0V0 is the answer.
option C is the right answer.

18) Efficiency = 1-T2/T1
T2 is the temperature of cold reservoir. T2 = 294 K
T1 is the temperature of hot reservoir

0.6 = 1-(294/T1)
294/T1 = 0.4
T1 = 294/0.4 = 735 K
option A is the right answer.

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