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A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.
Correct answer is '10'. Can you explain this answer?
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A calorimeter consists of 400 g of water at 24°C. A 500 g piece of...
°C. A 100 g piece of metal is heated to 100 °C and then dropped into the calorimeter. The final temperature of the mixture is 30 °C. Calculate the specific heat capacity of the metal.
To solve this problem, we can use the principle of conservation of energy. The heat gained by the water and the metal is equal to the heat lost by the metal.
The heat gained by the water can be calculated using the formula:
Qwater = mwater * cwater * ΔTwater
where:
Qwater = heat gained by water
mwater = mass of water = 400 g
cwater = specific heat capacity of water = 4.18 J/g°C (approximately)
ΔTwater = change in temperature of water = final temperature - initial temperature = 30 °C - 24 °C = 6 °C
Qwater = 400 g * 4.18 J/g°C * 6 °C
Qwater = 10032 J
The heat lost by the metal can be calculated using the formula:
Qmetal = mmetal * cmetal * ΔTmetal
where:
Qmetal = heat lost by metal
mmetal = mass of metal = 100 g
cmetal = specific heat capacity of metal (unknown)
ΔTmetal = change in temperature of metal = final temperature - initial temperature = 30 °C - 100 °C = -70 °C (negative because the metal loses heat)
Qmetal = 100 g * cmetal * -70 °C
Qmetal = -7000 cmetal
Since the heat gained by the water and the heat lost by the metal are equal, we can set up the equation:
Qwater = Qmetal
10032 J = -7000 cmetal
Solving for cmetal, we get:
cmetal = -10032 J / -7000
cmetal ≈ 1.43 J/g°C
Therefore, the specific heat capacity of the metal is approximately 1.43 J/g°C.
To solve this problem, we can use the principle of conservation of energy. The heat gained by the water and the metal is equal to the heat lost by the metal.
The heat gained by the water can be calculated using the formula:
Qwater = mwater * cwater * ΔTwater
where:
Qwater = heat gained by water
mwater = mass of water = 400 g
cwater = specific heat capacity of water = 4.18 J/g°C (approximately)
ΔTwater = change in temperature of water = final temperature - initial temperature = 30 °C - 24 °C = 6 °C
Qwater = 400 g * 4.18 J/g°C * 6 °C
Qwater = 10032 J
The heat lost by the metal can be calculated using the formula:
Qmetal = mmetal * cmetal * ΔTmetal
where:
Qmetal = heat lost by metal
mmetal = mass of metal = 100 g
cmetal = specific heat capacity of metal (unknown)
ΔTmetal = change in temperature of metal = final temperature - initial temperature = 30 °C - 100 °C = -70 °C (negative because the metal loses heat)
Qmetal = 100 g * cmetal * -70 °C
Qmetal = -7000 cmetal
Since the heat gained by the water and the heat lost by the metal are equal, we can set up the equation:
Qwater = Qmetal
10032 J = -7000 cmetal
Solving for cmetal, we get:
cmetal = -10032 J / -7000
cmetal ≈ 1.43 J/g°C
Therefore, the specific heat capacity of the metal is approximately 1.43 J/g°C.
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A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer?
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A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer?.
A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A calorimeter consists of 400 g of water at 24°C. A 500 g piece of copper at 100°C is thrown into the water and the equilibrium temperature is found to be 36.5°C. What is the molar heat capacity of copper in cal/mol k, given that 1 mol of copper has a mass of 63.5g? Neglect the heat capacity of the container.Correct answer is '10'. Can you explain this answer?.
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