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1. Ice (1.0 kg) at -10.0 °C is allowed to melt and warm to 25.0 °C,...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...
Two 20.0g ice cubes at -12.0^degree C are placed into 285g of water at 25.0^degree C....
Two 20.0g ice cubes at -12.0^degree C are placed into 285g of water at 25.0^degree C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of H2O(s) is 37.7 J/mol*K heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20 is 6.01 kJ/mol
I would really appreciate your help. God bless you Question 4 The molar enthalpy of fusion of ice at 0 °C and 1 atm...
I would really appreciate your help. God bless
you
Question 4 The molar enthalpy of fusion of ice at 0 °C and 1 atm pressure is 6024 J mol. The molar heat capacities at constant pressure of ice and water are 37.65 J Kmol and 75.30 J Kmol respectively, and may be taken as constant over the temperature range 0 to -20°C. Consider 2 mole of liquid water supercooled to -20 °C, which is allowed to freeze isothermally from liquid...
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed...
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K
5. If 100 g of water cooled to -6°C) is allowed to freeze at -6°C, what...
5. If 100 g of water cooled to -6°C) is allowed to freeze at -6°C, what is the entropy change? What is the entropy change of the surroundings? What is the entropy change of the universe? H2O() → H2O(1) AH = 6.008 kJ/mol Cp,solid = 33.8 J/(K mol) Cp.liquid = 75.3 J/(K mol)
The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is...
The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/g·K , 4.184 J/g·K , and 1.84 J/g·K respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap =40.67 kJ/mol
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at...
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T, of the water after all the ice melts. heat capacity of H2O(s) heat capacity of H2O(1) enthalpy of fusion of H,O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti =
If a 0.06250 kg ice cube initially at 0.000 C is allowed to melt in a...
If a 0.06250 kg ice cube initially at 0.000 C is allowed to melt in a Styrofoam cup holding 0.497 kg of water at 10.00 C , what is the total entropy change for this process?
1. Ice melts at 0C° with an enthalpy of fusion = 6.01 kJ mol-1 . An...
1. Ice melts at 0C° with an enthalpy of fusion = 6.01 kJ mol-1 . An ice cube with a mass of 20.0g is placed inside an incubator at 40.0C°. Determine the total entropy change (in J/K) of this system. 2. Calculate the total entropy change (in J/K) when 50.0 g of H2 gas initially in a tank at a pressure of 145 psi is withdrawn from the tank under a constant pressure of 23.0 psi at standard room temperature....
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at...
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T. of the water after all the ice melts. heat capacity of H,O() heat capacity of H,O(1) enthalpy of fusion of H,0 37.7J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti = 24.99 "C Incorrect
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...
I would really appreciate your help. God bless
you
Question 4 The molar enthalpy of fusion of ice at 0 °C and 1 atm pressure is 6024 J mol. The molar heat capacities at constant pressure of ice and water are 37.65 J Kmol and 75.30 J Kmol respectively, and may be taken as constant over the temperature range 0 to -20°C. Consider 2 mole of liquid water supercooled to -20 °C, which is allowed to freeze isothermally from liquid...
5. If 100 g of water cooled to -6°C) is allowed to freeze at -6°C, what is the entropy change? What is the entropy change of the surroundings? What is the entropy change of the universe? H2O() → H2O(1) AH = 6.008 kJ/mol Cp,solid = 33.8 J/(K mol) Cp.liquid = 75.3 J/(K mol)
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T, of the water after all the ice melts. heat capacity of H2O(s) heat capacity of H2O(1) enthalpy of fusion of H,O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti =
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T. of the water after all the ice melts. heat capacity of H,O() heat capacity of H,O(1) enthalpy of fusion of H,0 37.7J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti = 24.99 "C Incorrect
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