the water is at 55 °C. Now slowly add heat to the sample of liquid water until it freezes. What happens to the water as it freezes in terms of the strength of the bonds, the entropy of the system, and the types of motion that exist?
As heat is added to water, the thermal energy of molecules increases and then they vibrate with increased frequency. As a consequence of increased energetic vibrations,the bond between the water and molecule weakens resulting in the increase of bond length
The entropy of the system increases as the water release heat as it condenses.
When water freezes the molecules slows down and settle into place, lining up in regular formations.
the water is at 55 °C. Now slowly add heat to the sample of liquid water...
An ice tray contains 490 g of liquid water at 0°C. Calculate the change in entropy of the water as it freezes slowly and completely at 0°C. J/K
3. A piston-cylinder device initially contains 3 kg saturated liquid water at 500 kPa. Now heat is transferred to the water until the cylinder contains saturated vapor only. Determine water m = 3 kg p = 500 kPa a) The initial and final volume of the cylinder, b) The boundary work of the piston, and c) The heat added to the system
What is the change in entropy of 0.97 mol of liquid water at 0.0 degree C that freezes to ice at 0.0 degree C? J/K
A piston-cylinder device initially contains 1.78 kg saturated liquid water at 200°C. Now heat is transferred to the water until the volume quadruples and the cylinder contains saturated vapor only. Determine (a) the final volume of the tank, m (Round to six decimal places.) (b) the final temperature and pressure, MPa and (c) the internal energy change of the water kJ 0 Water 1.78 kg 200 C
What is the generated entropy (in kJ/K) when 1 kg of liquid water at 25°C is heated to saturated vapor at 100°C in an oven that is at 150°C. Hint: the effect of pressure on the entropy of liquids or solids is usually negligible. Now assume you are trying to heat 1 kg of liquid water at 25°C to saturated vapor at 100°C, but you want to do it in an oven that is at 80°C. This is obviously impossible...
A piston cylinder device initially contains 1.2kg of saturated liquid water at 220oC. Now, heat is transferred to the water until the volume quadruples and the cylinder contains saturated vapor only. Determine (a) the final volume of the tank, (b) the final temperature (c) the final pressure, and (d) the change in internal energy of the tank. To check your work, enter the final pressure in kPa in the box below. Also, sketch this process on a T-v diagram.
Consider converting 1.50 mol of ice at - 25 degree C to liquid water at 55 degree C at 1 atm. What calculation would give the quantity of heat required by this process in J? The molar heat capacity of ice is 37.6 mol^-1 degree C^-1. The molar heat capacity of liquid water is 75.4 J-mol^-1 degree C^-1. The heat of fusion of water is 6.02 kJ mol^-1. (A) q = (1.50 mol) (6.02 kJ/mol) (1000 J/kJ) (B) q =...
An insulated Thermos contains 135 g of water at 86.5 ˚C. You put in a 7.06 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An insulated Thermos contains 143 g of water at 82.8 ˚C. You put in a 9.07 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An insulated Thermos contains 116 g of water at 89.5 ˚C. You put in a 7.91 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?