Homework Answers
As the equilibrium temperature is 20 degree celcius,the water is neither loosing heat nor gaining.
So we can write,
Heat loss by Lead = heat gain by copper
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8. You have a large insulated container of water at 20°C. You place a 0.5kg 100°C...
Problem 5 20 points You place into an insulated container a 1.5 kg of copper initially...
Problem 5 20 points You place into an insulated container a 1.5 kg of copper initially at 70°C. You add to the insulated container water, initially at 20°C to obtain a final temperature of the system equal to 50°C. The specific heat of some materials are given in the table below: Aluminum Copper Material J/g/°C Glass Gold Ice Iron Rubber Silver Water zinc 0.79 0.13 2.1 0.46 0.24 4.2 0.39 0.89 0.38 2 a) [5 points) What is the variation...
A 20-g ice cube floats in 210 g of water in a 100-g copper cup; all...
A 20-g ice cube floats in 210 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 92°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C,...
Initially you have mW = 3.4 kg of water at TW = 54°C in an insulated container. You add ice at TI = -21°C to the contain...
Initially you have mW = 3.4 kg of water at
TW = 54°C in an insulated container. You add
ice at TI = -21°C to the container and the mix
reaches a final, equilibrium temperature of Tf
= 25°C. The specific heats of ice and water are
cI = 2.10×103J/(kg⋅°C) and
cW = 4.19×103 J/(kg⋅°C),
respectively, and the latent heat of fusion for water is
Lf = 3.34×105 J/kg.
(11%) Problem 7: Initially you have mw = 3.4 kg of...
Problem 7.30 You place into an insulated container a 1.8 kg block of aluminum at a...
Problem 7.30 You place into an insulated container a 1.8 kg block of aluminum at a temperature of 43°C in contact with a 2.4 kg block of copper at a temperature of 18°C. The specific heat of aluminum is 0.91 J/K/g and the specific heat of copper is 0.391/K/g, what is the final temperature of the two blocks? oC the tolerance is +/-296
What mass of ice would it take to lower the temperature of 0.5kg of water 20°C...
What mass of ice would it take to lower the temperature of 0.5kg of water 20°C to 0°C. 7. from A 100-g piece of iron is heated to 100°C and then dropped into a cavity in a large block ofice at 0°C. How much mass of ice will melt? 8. 50 grams of hot water at 80°C is poured into a cavity in a very large block ofice at 0°C. The final temperature of the water in the cavity is...
6. (20 pts) You have a beaker containing 100 mL of water. The initial temperature of...
6. (20 pts) You have a beaker containing 100 mL of water. The initial temperature of the water is 20°C. (Note: Onc ml = 1 cm'). 2. You place a piece of copper into the beakct containing. When you do, the water level increases to 110.5 m... What is the mass of the copper in grams? b. If the temperature of the water increases to 35°C, how much heat (in calories) did the copper add to the water? c. You...
A calorimeter is a container that is insulated from the outside, so a negligible amount of...
A calorimeter is a container that is insulated from the outside, so a negligible amount of energy enters or leaves the container when it is closed. Consider a copper calorimeter with mass 0.100 kg that contains 0.160 kg of water and 0.018 kg of ice, all in thermal equilibrium at atmospheric pressure. If 0.750 kg of lead at a temperature of 255 ∘C is dropped into the calorimeter, what is the final temperature? Assume that no heat is lost to...
A 38-g ice cube floats in 190 g of water in a 100-g copper cup; all...
A 38-g ice cube floats in 190 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 96°C is dropped into the cup, and the final equilibrium temperature is 12°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 105 J/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 and 387 J/kg · °C,...
Of ice at -S °C is added to 40 kg of water initially at 20 °C. Assume that the container is well ...
of ice at -S °C is added to 40 kg of water initially at 20 °C. Assume that the container is well insulated. (a) Find the final equilibrium temperature. (5 points) 0b) Caleulate the change in internal energy of the 40 kg water when thermal equilberium is established. (5 points) (c) If a 3 kg piece of copper at 30°C is also added to the original system( Le. system with ice d wat an (7 points) er at their initial...
(17%) Problem 6: You have mw = 4.9 kg of water in an insulated container. You...
(17%) Problem 6: You have mw = 4.9 kg of water in an insulated container. You add mı = 0.15 kg of ice at Ty=-19°C to the water and the mix reaches a final, equilibrium temperature of Tp = 11°C. The specific heats of ice and water are q = 2.10x10 J/(kg-ºC) and cw = 4.19x10 J/(kg:°C), respectively, and the latent heat of fusion for water is 4 = 3.34x10J/kg. Calculate the initial temperature of the water, in degrees Celsius....
Problem 5 20 points You place into an insulated container a 1.5 kg of copper initially at 70°C. You add to the insulated container water, initially at 20°C to obtain a final temperature of the system equal to 50°C. The specific heat of some materials are given in the table below: Aluminum Copper Material J/g/°C Glass Gold Ice Iron Rubber Silver Water zinc 0.79 0.13 2.1 0.46 0.24 4.2 0.39 0.89 0.38 2 a) [5 points) What is the variation...
Initially you have mW = 3.4 kg of water at
TW = 54°C in an insulated container. You add
ice at TI = -21°C to the container and the mix
reaches a final, equilibrium temperature of Tf
= 25°C. The specific heats of ice and water are
cI = 2.10×103J/(kg⋅°C) and
cW = 4.19×103 J/(kg⋅°C),
respectively, and the latent heat of fusion for water is
Lf = 3.34×105 J/kg.
(11%) Problem 7: Initially you have mw = 3.4 kg of...
Problem 7.30 You place into an insulated container a 1.8 kg block of aluminum at a temperature of 43°C in contact with a 2.4 kg block of copper at a temperature of 18°C. The specific heat of aluminum is 0.91 J/K/g and the specific heat of copper is 0.391/K/g, what is the final temperature of the two blocks? oC the tolerance is +/-296
What mass of ice would it take to lower the temperature of 0.5kg of water 20°C to 0°C. 7. from A 100-g piece of iron is heated to 100°C and then dropped into a cavity in a large block ofice at 0°C. How much mass of ice will melt? 8. 50 grams of hot water at 80°C is poured into a cavity in a very large block ofice at 0°C. The final temperature of the water in the cavity is...
6. (20 pts) You have a beaker containing 100 mL of water. The initial temperature of the water is 20°C. (Note: Onc ml = 1 cm'). 2. You place a piece of copper into the beakct containing. When you do, the water level increases to 110.5 m... What is the mass of the copper in grams? b. If the temperature of the water increases to 35°C, how much heat (in calories) did the copper add to the water? c. You...
of ice at -S °C is added to 40 kg of water initially at 20 °C. Assume that the container is well insulated. (a) Find the final equilibrium temperature. (5 points) 0b) Caleulate the change in internal energy of the 40 kg water when thermal equilberium is established. (5 points) (c) If a 3 kg piece of copper at 30°C is also added to the original system( Le. system with ice d wat an (7 points) er at their initial...
(17%) Problem 6: You have mw = 4.9 kg of water in an insulated container. You add mı = 0.15 kg of ice at Ty=-19°C to the water and the mix reaches a final, equilibrium temperature of Tp = 11°C. The specific heats of ice and water are q = 2.10x10 J/(kg-ºC) and cw = 4.19x10 J/(kg:°C), respectively, and the latent heat of fusion for water is 4 = 3.34x10J/kg. Calculate the initial temperature of the water, in degrees Celsius....
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