First Law for Closed Systems
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 The First Law for a closed system ensures conservation of:
Explanation: The First Law conserves energy, balancing internal energy, heat, and work in a closed system.
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 If a closed system loses 40 J of heat and does 20 J of work, ΔU is
Explanation: Heat loss means Q = -40 J. Using ΔU = Q – W, ΔU = -40 J – 20 J = -60 J
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A closed system’s internal energy depends on:
Explanation: Internal energy is a state (point) function, determined by properties like temperature and volume, not process.
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For a closed system with no heat or work exchange, ΔU is:
Explanation: If Q = 0 and W = 0, then ΔU = Q – W = 0, so internal energy remains constant.
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What cannot cross the boundary of a closed system?
Explanation: A closed system prevents mass transfer but allows energy transfer as heat or work.
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 If a closed system does 50 J of work and gains 80 J of heat, what is ΔU?
Explanation: Using ΔU = Q – W, ΔU = 80 J – 50 J = 30 J. Internal energy increases by 30 J.
7 / 10
In a closed system undergoing an adiabatic process (Q = 0), ΔU equals:
Explanation: For Q = 0, ΔU = Q – W = -W. Internal energy change is the negative of work done.
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 If 200 J of heat is added to a closed system with no work done, ΔU is:
Explanation: Using ΔU = Q – W, if Q = 200 J and W = 0, then ΔU = 200 – 0 = 200 J.
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A closed system is characterized by:
Explanation: A closed system allows heat and work exchange but no mass enters or leaves, unlike an open system.
10 / 10
For a closed system, the First Law is expressed as:
Explanation: In a closed system, internal energy change (ΔU) equals heat added (Q) minus work done by the system (W).
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