A piece of gold metal is heated from 25C to 90C. It is then dropped into...
A piece of gold metal is heated from 25C to 90C. It is then
dropped into 1 litre of water at 25.0 o C and the water temperature
increases to 25.4 o C. The heat capacity of gold is
0.129 J K-1 g -1 and that of water is 4.18 J K-1 g -1.
(A) what is the mass of gold sample
(b) what is the entropy change in the gold as it is heated up?
(c) assume that water stays constant what is the entropy change in the surround water when gold is added?
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A piece of gold metal is heated from 25C to 90C. It is then
dropped into...
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker...
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K). 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K) Previous Page Next Page Page 22 of 24 Submit Quiz 0 of 24 questions saved
A piece of copper metal is initially at 83.0°C. It is dropped into a coffee cup...
A piece of copper metal is initially at 83.0°C. It is dropped into a coffee cup calorimeter containing 30.0 9 of water at a temperature of 10.0°c. After stirring, the final temperature of both copper and water is 25.0°c. Assuming no heat losses, and that the specific heat (capacity) of water is 4.18 J/(g.), what is the heat capacity of the copper in J/K?
A piece of metal having a density of 19.3 g/mL when dropped into a graduated cylinder...
A piece of metal having a density of 19.3 g/mL when dropped into a graduated cylinder containing 50 mL of water the reading was 61.3 mL. When the metal was heated from 25°C to 50°C the heating required 703.34 joules of heat. What is the heat capacity of the metal? O 0.129 J/g-°C O 1.29 J/g-°C 0 0.024 J/g-°C O 0.24 J/g-°C 0 2.40 J/g-°C
A 29.3 g piece of metal is heated to 97 degree C and dropped into a...
A 29.3 g piece of metal is heated to 97 degree C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g degree C) initially at 22.9 degree C. The empty calorimeter has a heat capacity of 125 J/K. the final temperature of the water is 25.96 degree C. Ignoring significant figures., calculate the specific heat of the metal. A) 0.481 J/gK. B) 0.361 J/gK C) 0.120 J/gK D) 0.300 J/gK E)...
A 75.0 g piece of Au metal is heated to 80.0 ∘Cand dropped into 50.0 g...
A 75.0 g piece of Au metal is heated to 80.0 ∘Cand dropped into 50.0 g of water at 23.2 ∘C. The final temperature of the Au−H2O mixture is 25.7 ∘C. What is the specific heat capacity of gold? Express your answer in joules per grams degrees Celsius to three significant figures.
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then...
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K) 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K)
21.A piece of copper metal is initially at 100 C. It is dropped into a coffee...
21.A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0g of water at a temperature of 20.0°C. After thermal equilibrium established, the final temperature of both copper and water is 25.0 °C. Assume there is no heat loss what is the heat capacity, C, of the copper? The specific heat of water is 4.18 J/g°C tutor a. 2.79 J/oC b. 3.33 JoC c. 2.79 J/oC d. 13.9 JoC 3
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10...
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00...
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
9. A 48.8 g piece of an unknown metal was heated to 99.8°C, then dropped into...
9. A 48.8 g piece of an unknown metal was heated to 99.8°C, then dropped into a coffee cup calorimeter containing 40.0 g of water at 26.3°C The temperature of the water increased to 30.2°C. How much heat flowed into the water? What is the specific heat of the unknown metal?
A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K). 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K) Previous Page Next Page Page 22 of 24 Submit Quiz 0 of 24 questions saved
A piece of copper metal is initially at 83.0°C. It is dropped into a coffee cup calorimeter containing 30.0 9 of water at a temperature of 10.0°c. After stirring, the final temperature of both copper and water is 25.0°c. Assuming no heat losses, and that the specific heat (capacity) of water is 4.18 J/(g.), what is the heat capacity of the copper in J/K?
A piece of metal having a density of 19.3 g/mL when dropped into a graduated cylinder containing 50 mL of water the reading was 61.3 mL. When the metal was heated from 25°C to 50°C the heating required 703.34 joules of heat. What is the heat capacity of the metal? O 0.129 J/g-°C O 1.29 J/g-°C 0 0.024 J/g-°C O 0.24 J/g-°C 0 2.40 J/g-°C
A 29.3 g piece of metal is heated to 97 degree C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g degree C) initially at 22.9 degree C. The empty calorimeter has a heat capacity of 125 J/K. the final temperature of the water is 25.96 degree C. Ignoring significant figures., calculate the specific heat of the metal. A) 0.481 J/gK. B) 0.361 J/gK C) 0.120 J/gK D) 0.300 J/gK E)...
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K) 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K)
21.A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0g of water at a temperature of 20.0°C. After thermal equilibrium established, the final temperature of both copper and water is 25.0 °C. Assume there is no heat loss what is the heat capacity, C, of the copper? The specific heat of water is 4.18 J/g°C tutor a. 2.79 J/oC b. 3.33 JoC c. 2.79 J/oC d. 13.9 JoC 3
9. A 48.8 g piece of an unknown metal was heated to 99.8°C, then dropped into a coffee cup calorimeter containing 40.0 g of water at 26.3°C The temperature of the water increased to 30.2°C. How much heat flowed into the water? What is the specific heat of the unknown metal?
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