Suppose that there are two very large reservoirs of water, one at a temperature of 85.0 °C and one at a temperature of 19.0 °C. These reservoirs are brought into thermal contact long enough for 35850 J of heat to flow from the hot water to the cold water. Assume that the reservoirs are large enough so that the temperatures do not change significantly. What is the total change in entropy, AStot, resulting from this heat exchange between the hot water and the cold water? AStot = J/K Calculate the amount of energy made unavailable for work by this increase in entropy. amount of energy unavailable for work: J How much work could a Carnot engine do if it took in the given amount of heat (35850 J) from the hot water reservoir and exhausted heat to the cold water reservoir? work done by a Carnot engine:

Suppose that there are two very large reservoirs of water, one at a temperature of 85.0 °C and one at a temperature of 19.0 °C. These reservoirs are brought into thermal contact long enough for 35850 J of heat to flow from the hot water to the cold water. Assume that the reservoirs are large enough so that the temperatures do not change significantly. What is the total change in entropy, AStot, resulting from this heat exchange between the hot water and the cold water? AStot = J/K Calculate the amount of energy made unavailable for work by this increase in entropy. amount of energy unavailable for work: J How much work could a Carnot engine do if it took in the given amount of heat (35850 J) from the hot water reservoir and exhausted heat to the cold water reservoir? work done by a Carnot engine:

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

A) 20 J of heat is transferred from a hotter reservoir to a colder reservoir. Calculate ΔStot (J K-1) when the hotter reservoir is at 10 °C and the colder is at 0 °C. B) Calculate ΔStot (J K-1) when 10 J of heat flows reversibly from a 100 °C reservoir to another 100 °C reservoir. C)The change in total entropy is positive when heat is transferred between a hot object and a cold object in thermal contact because the process is irreversible. True or false?
Two objects which is the B1 (T = 40 C) and B2 (T = 18 C), has experienced entropy changes of 6.4 x 104 J/K and 2.8 x 104 J/K, respectively after they had been placed in direct contact with each other. B1 has lost 2.0 x107 J of heat. How much heat was lost by B2? What was the entropy change in the universe after the process?
Suppose we place 50 g of ice at 0 °C in contact with a heat reservoir at 20 °C . Heat spontaneously flows from the reservoir to the ice, which melts and eventually reaches a temperature of 20 °C . Find the change in entropy of (a) the ice and (b) the universe.
A freezer is used to freeze 5.0 L of water completely into ice. The water and the freezer remain at a constant temperature of T = 0°C. (a) Determine the change in the entropy of the water. kJ/K (b) Determine the change in the entropy of the freezer. kJ/K
Qs b and c
Suppose 1.00 kg of water at 100C is placed in thermal contact with 1.00 kg of water at 0C. What is the total change in entropy? Assume that the specific heat of water is constant at 4190 J/kg . K over this temperature range.
An ice tray contains 500 g of water. Calculate the change in entropy of the water as it freezes completely and slowly at 0 oC.
What is the decrease in entropy of 25.0 g of water that condenses on a bathroom mirror at a temperature of 35.0C, assuming no change in temperature and given the latent heat of vaporization to be 2450 kJ/kg?
A puddle containing 1.10 kg of water at 0°C freezes on a cold night, becoming ice at 0°C. What was the entropy change of the water that is now ice? (The latent heat of freezing water is 333 J / K.) The change in entropy is
A tank of 100-g liquid water at 100°C is put in thermal contact with another tank of 300-g water at 30°C. These two tanks are insulated from the outside so that heat can be exchanged only between these two tanks. Please compute the entropy change in each tank, and the total entropy change.
It takes about 335 J to melt one gram of ice. During the melting, the temperature stays constant. Which has higher entropy, a gram of liquid water at 0 degree Celcius or a gram of ice at 0 degree Celcius? Does this make sense? How large is the entropy difference?
A 500-g chocolate bar starts to melt at 45OC. What is the change in entropy? (Note: The latent heat of fusion of chocolate Lf = 1.5 x 105 J/kg. Calculate first the heat needed to melt the chocolate using the formula Q = mLf, where Q is the amount of heat needed to melt the chocolate, m is the mass of the chocolate, and Lf is the latent heat of fusion of chocolate.)