Answer :
Final answer:
The change in internal energy of a system, ΔE, considering 750 J of work done on the system and 195 J of heat given off by the system, is 555 J according to the first law of thermodynamics. Option 3 is the correct answer.
Explanation:
This question deals with the concept of internal energy in a system, which is represented by ΔE. In the given problem, there is 750 J of work done on the system and the system gives off 195 J of heat. To find the change in internal energy, one can apply the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system plus the work done on the system. In equation form, this is represented as ΔE = Q + W.
In the given context, heat 'given off' by the system equates to negative heat input (Q), hence this value will be taken as -195 J. The work done on the system is +750 J. Plugging in these values into the formula, we get ΔE = -195 J + 750 J = 555 J. Therefore, the correct answer is 3) 555 J.
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