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13. The temperature of 150.0 g of zinc is lowered from 25.0°C to 16.4 C as...
Liquid nitrogen is often used as an effective coolant, as its boiling temperature is far below...
Liquid nitrogen is often used as an effective coolant, as its boiling temperature is far below the freezing temperature of water. Specifically, the boiling point of liquid nitrogen is 77.0 K. A 0.650-kg block of iron at an initial temperature of 293.15 K is immersed in an insulated bath of liquid nitrogen with an initial temperature of 77.0 K. After the iron and the liquid nitrogen reach a state of thermal equilibrium, the iron block has cooled to a final...
(3) Use the vapor pressures for tetrachloromethane given in the following table to estimate the temperature...
(3) Use the vapor pressures for tetrachloromethane given in the following table to estimate the temperature and pressure of the triple point and also the enthalpies of fusion, vaporization and sublimation. Solid 230 225.7 280 340 6440 62501 Liquid 4) Calculate the change in the freezing point of water at 100. and 500. bar compared to that at 1 bar assuming that the density of the liquid and solid phases remain constant at 997 and 917 kg m, respectively. Explain...
A 150.0-g glass beaker contains 750 g of water initially at 25.0 degree C. A 250.0-g...
A 150.0-g glass beaker contains 750 g of water initially at 25.0 degree C. A 250.0-g piece of copper is taken out of a hot oven and dropped into the water. After equilibrium is reached between the copper, glass, and water, the final 'temperature is 32.0 degree C. What was the temperature of the oven?
Calculate the amount of heat (in kJ) required to raise the temperature of 14.0 g of...
Calculate the amount of heat (in kJ) required to raise the temperature of 14.0 g of liquid H_2O (molar mass = 18.0 g/mol) from 25.0 degree C to the boiling point and then to vaporize the liquid at that temperature, (specific heal capacities: H_2O(s): 2.06 J/g degree C, H_2O(l): 4.18 J/g degree C, H_2O(g): 1.92 J/g degree C; heat of fusion of H_2O: 6.02 kJ/mol; heat of vaporization of H_2O: 40.7 kJ/mol; melting point of H_2O: 0.0 degree C, boiling...
Calculate the total quantity of heat required to convert 25.0 g of liquid CCl 4 (...
Calculate the total quantity of heat required to convert 25.0 g of liquid CCl 4 ( l ) from 35.0°C to gaseous CCl 4 at 76.8°C (the normal boiling point for CCl 4 ). The specific heat of CCl 4 ( l ) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol.
1. How much energy (in kilojoules) is released when 16.4 g of steam at 116.5 ∘C...
1. How much energy (in kilojoules) is released when 16.4 g of steam at 116.5 ∘C is condensed to give liquid water at 60.5 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor. 2.What is the entropy of fusion, ΔSfusion [in J/(K⋅mol)] for sodium? The necessary data are the following: mp = 97.8 ∘C,bp = 883 ∘C, ΔHvap = 89.6kJ/mol, and...
A 150.0-g sample of metal at 80.0°C is added to 150.0 g of H20 at 20.0°C....
A 150.0-g sample of metal at 80.0°C is added to 150.0 g of H20 at 20.0°C. The temperature rises to 23.3°C. Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal? (Specific heat of H2O is 4.18 J/g. °C.) A) -0.48 J/g. °C B) 0.24 J/g °C C) 0.48 J/g °C D) 0.72 J/g °C E) 0.96 J/g. "C
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0...
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
. A 150.0 g sample of a Metal was heated to 95.0°C. When the hot metal...
. A 150.0 g sample of a Metal was heated to 95.0°C. When the hot metal was placed into 100.0 g of water in a calorimeter, the temperature of the water increased from 20.0°C to 35.0°C. The specific heat of water is 4.184 J/g °C. a) What is the specific heat of the metal? Kb) What would the final temperature be if the mass of water was 150.0 q?
A 57.1 g piece of zinc (Csp = 0.388 J/g · °C), initially at 285.8 °C,...
A 57.1 g piece of zinc (Csp = 0.388 J/g · °C), initially at 285.8 °C, is added to 155.3 g of a liquid, initially at 22.1 °C, in an insulated container. The final temperature of the metal–liquid mixture at equilibrium is 36.7 °C. What is the identity of the liquid? Neglect the heat capacity of the container.
Liquid nitrogen is often used as an effective coolant, as its boiling temperature is far below the freezing temperature of water. Specifically, the boiling point of liquid nitrogen is 77.0 K. A 0.650-kg block of iron at an initial temperature of 293.15 K is immersed in an insulated bath of liquid nitrogen with an initial temperature of 77.0 K. After the iron and the liquid nitrogen reach a state of thermal equilibrium, the iron block has cooled to a final...
(3) Use the vapor pressures for tetrachloromethane given in the following table to estimate the temperature and pressure of the triple point and also the enthalpies of fusion, vaporization and sublimation. Solid 230 225.7 280 340 6440 62501 Liquid 4) Calculate the change in the freezing point of water at 100. and 500. bar compared to that at 1 bar assuming that the density of the liquid and solid phases remain constant at 997 and 917 kg m, respectively. Explain...
A 150.0-g glass beaker contains 750 g of water initially at 25.0 degree C. A 250.0-g piece of copper is taken out of a hot oven and dropped into the water. After equilibrium is reached between the copper, glass, and water, the final 'temperature is 32.0 degree C. What was the temperature of the oven?
Calculate the amount of heat (in kJ) required to raise the temperature of 14.0 g of liquid H_2O (molar mass = 18.0 g/mol) from 25.0 degree C to the boiling point and then to vaporize the liquid at that temperature, (specific heal capacities: H_2O(s): 2.06 J/g degree C, H_2O(l): 4.18 J/g degree C, H_2O(g): 1.92 J/g degree C; heat of fusion of H_2O: 6.02 kJ/mol; heat of vaporization of H_2O: 40.7 kJ/mol; melting point of H_2O: 0.0 degree C, boiling...
A 150.0-g sample of metal at 80.0°C is added to 150.0 g of H20 at 20.0°C. The temperature rises to 23.3°C. Assuming that the calorimeter is a perfect insulator, what is the specific heat of the metal? (Specific heat of H2O is 4.18 J/g. °C.) A) -0.48 J/g. °C B) 0.24 J/g °C C) 0.48 J/g °C D) 0.72 J/g °C E) 0.96 J/g. "C
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
. A 150.0 g sample of a Metal was heated to 95.0°C. When the hot metal was placed into 100.0 g of water in a calorimeter, the temperature of the water increased from 20.0°C to 35.0°C. The specific heat of water is 4.184 J/g °C. a) What is the specific heat of the metal? Kb) What would the final temperature be if the mass of water was 150.0 q?
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