Chapter 20: Problem 13
Why might a heat pump have an advantage over a space heater that converts electrical energy directly into thermal energy?
Chapter 20: Problem 13
Why might a heat pump have an advantage over a space heater that converts electrical energy directly into thermal energy?
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Get started for freeFind the net change in entropy when \(100 . \mathrm{g}\) of water at \(0^{\circ} \mathrm{C}\) is added to \(100 . \mathrm{g}\) of water at \(100 .{ }^{\circ} \mathrm{C}\)
An inventor claims that he has created a water-driven engine with an efficiency of 0.200 that operates between thermal reservoirs at \(4^{\circ} \mathrm{C}\) and \(20 .{ }^{\circ} \mathrm{C}\). Is this claim valid?
The change in entropy of a system can be calculated because a) it depends only on the c) entropy always increases. initial and final states. d) none of the above. b) any process is reversible.
Assume that it takes \(0.0700 \mathrm{~J}\) of energy to heat a \(1.00-\mathrm{g}\) sample of mercury from \(10.000^{\circ} \mathrm{C}\) to \(10.500{ }^{\circ} \mathrm{C}\) and that the heat capacity of mercury is constant, with a negligible change in volume as a function of temperature. Find the change in entropy if this sample is heated from \(10 .{ }^{\circ} \mathrm{C}\) to \(100^{\circ} \mathrm{C}\).
1 .00 mole of a monatomic ideal gas at a pressure of 4.00 atm and a volume of \(30.0 \mathrm{~L}\) is isothermically expanded to a pressure of 1.00 atm and a volume of \(120.0 \mathrm{~L}\). Next, it is compressed at a constant pressure until its volume is \(30.0 \mathrm{~L}\), and then its pressure is increased at the constant volume of \(30.0 \mathrm{~L}\). What is the efficiency of this heat engine cycle?
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