When an aluminum bar is connected between a hot reservoir at 660 K and a cold reservoir at 318 K, 2.30 k) of energytransferred by heat from the hot reservoir to the cold reservoir.(a) In this irreversible process, calculate the change in entropy of the hot reservoir.(b) In this irreversible process, calculate the change in entropy of the cold reservoir.(c) In this irreversible process, calculate the change in entropy of the Universe, neglecting any change in entropy of the aluminum rod.

The temperature of the hot reservoir TH = 660 K The temperature of the cold reservoir TC = 318 K…

Answered: When an aluminum bar is connected…

Similar questions

What is the change in entropy in an adiabatic process? Does this imply that adiabatic processes are reversible? Can a process be precisely adiabatic for a macroscopic system?
A quantity of an ideal gas in an isolated system expanded isothermally and reversibly at 400 K from a volume V1 to a volume V2. During the expansion, the gas absorbs 200 cal of heat from the reservoir in contact with it.Calculate (a) the entropy change of the gas;(b) the entropy change of the reservoir, and(c) the entropy change of the whole system. units should be in j/k, (0.50, -0.50, 0)
Consider a 50.0 g ice cube placed in a container containing 200 g of water. The water is initially at 25.0*C and the ice cube comes directly from a freezer at -15.0*C. Assume no heat is lost to the surroundings and negligible heat loss from the container. Determine the total change in entropy as a result of the mixing process.
Some gas was compressed isothermally. This process was accompanied by a decrease in entropy (S=10 JK-1). Calculated the volume of the gas if it initially occupied the volume of 15.0 dm3 at 1.00 atm and 250 K. Does this violate the 2nd law of the thermodynamics stating that “the entropy of the isolated system can not decrease” ? Explain why.
Suppose you put a cube of ice of mass 100 g into a glass of water at just above 0°C. When the ice melts, about 33 kJ of energy is absorbed from the surroundings as heat. What is the change in entropy of (a) the sample (the ice) and (b) the surroundings (the glass of water)?
What is the change in entropy in converting 1.0 kg of ice at 0.0 degree celsius to 1.0 kg water at 0.0 degree celsius?
A heat source generates heat at a rate of 63.0 W (1 W=1 J/s). How much entropy does this produce per hour in the surroundings at 27.2 ∘C Assume the heat transfer is reversible.
Calculate the entropy of rolling a die three times such that the sum of numbers for the first two observations is divisible by the number obtained third time. (a) 6.47 x103 J/K (b) 2.03 m -kg-s.K (c) 2.81 m² - kg -s. K (d) 2.81x10-3 J/K
A 100-lbm block of a solid material whose specific heat is 0.5 Btu/lbm·R is at 80°F. It is heated with 10 lbm of saturated water vapor that has a constant pressure of 20 psia. Determine the final temperature of the block and water, and the entropy change of the entire system. Is this process possible? Why?