8) A block of copper (Cp,m = 24.44 J K-1 mol-1 ) of mass 2.00 kg...
8) A block of copper (Cp,m = 24.44 J K-1 mol-1 ) of mass 2.00 kg at 0 ℃ is introduced into an insulated container in which there is 1.00 mol H2O(g) at 100 ℃ and 1.00 atm. Assuming that all the vapour is condensed to liquid water, determine: (a) the final temperature of the system; (b) the heat transferred to the copper block; and (c) the entropy change of the water, the copper block, and the total system.
>> Can you please explain each step, and how we are able to determine the relationships. Thank you
Homework Answers
![Answire Giver (p, m (For copper) = 24.44 ] K1 molt Cp, m (For water) = 75. 348 JK mot! cy, water = 40. 66 kJ mo!!! = 60, 660](http://img.homeworklib.com/questions/cb524840-6fea-11ea-b9f0-8194c9cbe30f.png?x-oss-process=image/resize,w_560)
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C...
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C is added to 1.0 kg liquid water at 80 °C in an insulated container at constant atmospheric pressure. The copper has a heat capacity of 0.01 kJ kg1 and the specific heat of water is 4.2 kJ kg1 K (both assumed constant with temperature) c) Calculate the change in entropy of the system in b). s it appropriate to...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90 L of water at 10'C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp=418 kJ/kg-K. The density of water is 997 kg/m2. The specific heat of copper at 27°C is Cp=0.386 kJ/kg.K. Water Copper 90 L The final equilibrium temperature is OK The total entropy change during this process is OKJ/K.
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains...
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is Cp= 4.18 kJ/kg-K. The density of water is 997 kg/m3. The specific heat of copper at 27°C is cp=0.386 kJ/kg-K. Water Copper 90 L The final equilibrium temperature is 15.85 K. The total entropy change during this...
The constant-pressure molar heat capacity of H2O (s) and H2O (l) is 75.291 J K−1 mol−1...
The constant-pressure molar heat capacity of H2O (s) and H2O (l) is 75.291 J K−1 mol−1 and that of H2O (g) is 33.58 J K−1 mol−1 . Assume that the constant-pressure molar heat capacities are constant over the studied temperature range. Calculate the change in entropy of the system when 15.0 g of ice at −12.0 °C is converted to water vapour at 105.0 °C at a constant pressure of 1 bar!
You Answered Correct Answer Your answer is partially correct. A374 g block of copper whose temperature...
You Answered Correct Answer Your answer is partially correct. A374 g block of copper whose temperature is 305 K is placed in an insulating box with a 568 g block of lead whose temperatureis 189 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...
A block of iron ore A of mass m = 350 kg and specific heat capacity...
A block of iron ore A of mass m = 350 kg and specific heat capacity C = 460 kJ/(kg·K) obeys the constitutive relations where T is temperature. The block of metal is initially at temperature T1 = 700 K and it is placed in a perfectly-sealed, constant-pressure container B containing 64 kg of air initially at 320 K and atmospheric pressure 101.3 kPa. The air in container B can be modeled as a perfect gas with specific heat capacity...
The Standard enthalpy of vaporization of water at 100.0 oC is 40.66 KJ*mol-1. The Cp,m values for the liquid and the vap...
The Standard enthalpy of vaporization of water at 100.0
oC is 40.66 KJ*mol-1. The Cp,m
values for the liquid and the vapor water are, respectively, 75.3
and 33.58 J*K-1*mol-1. Assume that the heat
capacities are independent of temperature, and that the vapor
behaves as an ideal gas.
a) Calculate
sys in taking one mole of liquid water at 25.0
oC and 1.00 atm to gaseous water at 95.0 oC
and 0.500 atm.
b) Assume that the temperature and pressure of...
i got this question wrong. the book previously said that the units of entropy are J/(mol*K)....
i got this question wrong. the book previously said that the
units of entropy are J/(mol*K). you can get mol with the grams that
they gave, so why not use it?
Example: If, in a reversible process, 6.66 x 10 J of heat is used to change a 200 g block of ice to water at a temperature of 273 K, what is the change in the entropy of the system? (Note: The heat of fusion of ice = 333...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol)...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
1. A gas (1.00 mol) obeying the following equation of state (EOS) is compressed from P = 1.00 atm to P = 2.00 atm isoth...
1. A gas (1.00 mol) obeying the following equation of state (EOS) is compressed from P = 1.00 atm to P = 2.00 atm isothermally (300K) and reversibly: nRT P = v nb (a) (5 points) Calculate the entropy change, AS. (b) (10 points) Calculate the amount of heat () and work (w) involved. What does the total energy change (AU) tell you about the internal energy of this system?
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C is added to 1.0 kg liquid water at 80 °C in an insulated container at constant atmospheric pressure. The copper has a heat capacity of 0.01 kJ kg1 and the specific heat of water is 4.2 kJ kg1 K (both assumed constant with temperature) c) Calculate the change in entropy of the system in b). s it appropriate to...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90 L of water at 10'C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp=418 kJ/kg-K. The density of water is 997 kg/m2. The specific heat of copper at 27°C is Cp=0.386 kJ/kg.K. Water Copper 90 L The final equilibrium temperature is OK The total entropy change during this process is OKJ/K.
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is Cp= 4.18 kJ/kg-K. The density of water is 997 kg/m3. The specific heat of copper at 27°C is cp=0.386 kJ/kg-K. Water Copper 90 L The final equilibrium temperature is 15.85 K. The total entropy change during this...
You Answered Correct Answer Your answer is partially correct. A374 g block of copper whose temperature is 305 K is placed in an insulating box with a 568 g block of lead whose temperatureis 189 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...
The Standard enthalpy of vaporization of water at 100.0
oC is 40.66 KJ*mol-1. The Cp,m
values for the liquid and the vapor water are, respectively, 75.3
and 33.58 J*K-1*mol-1. Assume that the heat
capacities are independent of temperature, and that the vapor
behaves as an ideal gas.
a) Calculate
sys in taking one mole of liquid water at 25.0
oC and 1.00 atm to gaseous water at 95.0 oC
and 0.500 atm.
b) Assume that the temperature and pressure of...
i got this question wrong. the book previously said that the
units of entropy are J/(mol*K). you can get mol with the grams that
they gave, so why not use it?
Example: If, in a reversible process, 6.66 x 10 J of heat is used to change a 200 g block of ice to water at a temperature of 273 K, what is the change in the entropy of the system? (Note: The heat of fusion of ice = 333...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
1. A gas (1.00 mol) obeying the following equation of state (EOS) is compressed from P = 1.00 atm to P = 2.00 atm isothermally (300K) and reversibly: nRT P = v nb (a) (5 points) Calculate the entropy change, AS. (b) (10 points) Calculate the amount of heat () and work (w) involved. What does the total energy change (AU) tell you about the internal energy of this system?
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