150 g liquid water at 80.0°C is placed in an insulated flask. A 12.0 g ice cube at 0°C is added to the water in the flask to form a system of ice + water. (a) What is the equilibrium temperature of the system? (b) What is the net entropy change of the ice + water system as it reaches equilibrium? Data for the physical properties of water are available on the formula sheet.

150 g liquid water at 80.0°C is placed in an insulated flask. A 12.0 g ice cube at 0°C is added to the water in the flask to form a system of ice + water. (a) What is the equilibrium temperature of the system? (b) What is the net entropy change of the ice + water system as it reaches equilibrium? Data for the physical properties of water are available on the formula sheet.

Similar questions

A 23.9 g block of copper whose temperature is 382 K is placed in an insulating box with a 57.3 g block of lead whose temperature is 228 K. (a) What is the equilibrium temperature of the two-block system? (b) What is the change in the internal energy of the two-block system between the initial state and the equilibrium state? (c) What is the change in the entropy of the two-block system? The heat capacities of copper and lead are 386 J/kg-K and 128 J/kg-K, respectively. (a) Number i (b) Number i (c) Number i Units Units Units
For ice melting into water at 0 °C, the latent heat of fusion is Lp = 3.34 x 105 J/kg. For water boiling at 100 °C, the latent heat of vaporization is Ly = 2.26 x 105 J/kg. Which process involves a greater change in entropy? O melting 1.00 kg of ice at 0 °C O vaporizing 1.00 kg of liquid water at 100 °C the entropy change is the same for both
What is the decrease in entropy of 44.8 g of water that condenses on a bathroom mirror at a temperature of 39.7°C, assuming no change in temperature and given the latent heat of vaporization to be 2450 kJ/kg? Select the correct answer O 396 J/K O 189 J/K X Your Answer O 209 J/K 351 J/K O 251 J/K
A large factory furnace maintained at 170 ∘C at its outer surface is wrapped in an insulating blanket of thermal conductivity 5.50×10−2 W/(m⋅K) which is thick enough that the outer surface of the insulation is at 43.0 ∘C while heat escapes from the furnace at a steady rate of 140 W for each square meter of surface area. By how much does each square meter of the furnace change the entropy of the factory every second?
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?