One gram of supercooled liquid zinc at 400 °C is in a container of large heat capacity. Find the entropy change of zinc during solidification Zn(s) Cp=22.4 + 0.01005 J/molk AHm= 7388 J/mole at 420 °C Zn(I) Cp= 31.4 J/molK

One mole of a monoatomic ideal gas initially has a volume of 24.4L at latm and 298K undergoes a cyclic process as shown in Figure 6. Process 2→3 is an adiabatic expansion and process 3→1 is an isothermal compression. Given the V3 = 138L and T2 = 596K 2 1 3 Volume Figure 6 Calculate (a) the internal energy change in the process 1>2 (b) the entropy change in the process 1→2 (c) the heat released in the process 3->1 (d) the internal energy for one complete cycle 1→2→3→1. (e) the total work done for the entire process. Pressure

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 entropy change for 3.20 mol of an ideal monatomic gas undergoing a reversible increase in temperature from 380 K to 425 K at constant volume?