During an isothermal expansion, a confined ideal gas does –150 J of work against its surroundings. This implies that(a) 150 J heat has been removed from the gas(b) 300 J of heat has been added to the gas(c) no heat is transferred because the process is isothermal(d) 150 J of heat has been added to the gas
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This implies that 150J was added to the gas
Because the expansion is isothermal, no change in temperature occurs, which implies that no change in the internal energy of the gas takes place. Since ΔU =Q + W (the first law of thermodynamics), the fact that ΔU = 0 implies that Q = -W. Since W = -150 J, it must be true that Q = +150 J.
Because the expansion is isothermal, no change in temperature occurs, which implies that no change in the internal energy of the gas takes place. Since ΔU =Q + W (the first law of thermodynamics), the fact that ΔU = 0 implies that Q = -W. Since W = -150 J, it must be true that Q = +150 J.
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