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The internal energy change in a system that has absorbed 2 kcals of heat and done 500 J of work is: [2009]
  • a)
    6400 J
  • b)
    5400 J
  • c)
    7900 J
  • d)
    8900 J 
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
The internal energy change in a system that has absorbed 2 kcals of he...
According to first law of thermodynamics    Q = ΔU + W
ΔU = Q – W
       = 2 × 4.2 × 1000 – 500 = 8400 –500
       = 7900 J
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The internal energy change in a system that has absorbed 2 kcals of he...
To determine the internal energy change in a system, we need to consider the heat absorbed and the work done by the system.

Given:
Heat absorbed = 2 kcals (1 kcal = 4184 J)
Work done = 500 J

Converting heat absorbed from kcal to J:
2 kcals * 4184 J/kcal = 8368 J

Calculating the internal energy change:
Internal energy change = Heat absorbed - Work done
Internal energy change = 8368 J - 500 J
Internal energy change = 7868 J

Thus, the internal energy change in the system is 7868 J.

Summary:
- Heat absorbed = 2 kcals = 8368 J
- Work done = 500 J
- Internal energy change = Heat absorbed - Work done
- Internal energy change = 8368 J - 500 J = 7868 J

Therefore, the correct answer is option 'C' (7900 J).
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The internal energy change in a system that has absorbed 2 kcals of heat and done 500 J of work is: [2009]a)6400 Jb)5400 Jc)7900 Jd)8900 JCorrect answer is option 'C'. Can you explain this answer?
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