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19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1 (oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1
- a)0o C
- b)− 5o C
- c)5o C
- d)10o C
Correct answer is option 'C'. Can you explain this answer?
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19g of water at 30oC and 5g of ice at − 20oC are mixed together ...
0oC are mixed together. What is the final temperature of the mixture?
First, we need to calculate how much heat is required to melt the ice:
Q = m * Lf
Where Q is the heat required, m is the mass of the ice, and Lf is the specific heat of fusion for water, which is 334 J/g.
Q = 5g * 334 J/g = 1670 J
This means that 1670 J of heat energy is required to melt the ice.
Next, we need to calculate how much heat energy is required to raise the temperature of the water:
Q = m * Cp * ΔT
Where Q is the heat energy required, m is the mass of the water, Cp is the specific heat capacity of water, which is 4.18 J/g°C, and ΔT is the change in temperature.
Q = 19g * 4.18 J/g°C * (Tf - 30°C)
Where Tf is the final temperature of the mixture.
Now we can set the heat energy required to melt the ice equal to the heat energy required to raise the temperature of the water:
1670 J = 19g * 4.18 J/g°C * (Tf - 30°C)
Simplifying this equation:
Tf - 30°C = 1670 J / (19g * 4.18 J/g°C)
Tf - 30°C = 20.5°C
Tf = 50.5°C
Therefore, the final temperature of the mixture is 50.5°C.
First, we need to calculate how much heat is required to melt the ice:
Q = m * Lf
Where Q is the heat required, m is the mass of the ice, and Lf is the specific heat of fusion for water, which is 334 J/g.
Q = 5g * 334 J/g = 1670 J
This means that 1670 J of heat energy is required to melt the ice.
Next, we need to calculate how much heat energy is required to raise the temperature of the water:
Q = m * Cp * ΔT
Where Q is the heat energy required, m is the mass of the water, Cp is the specific heat capacity of water, which is 4.18 J/g°C, and ΔT is the change in temperature.
Q = 19g * 4.18 J/g°C * (Tf - 30°C)
Where Tf is the final temperature of the mixture.
Now we can set the heat energy required to melt the ice equal to the heat energy required to raise the temperature of the water:
1670 J = 19g * 4.18 J/g°C * (Tf - 30°C)
Simplifying this equation:
Tf - 30°C = 1670 J / (19g * 4.18 J/g°C)
Tf - 30°C = 20.5°C
Tf = 50.5°C
Therefore, the final temperature of the mixture is 50.5°C.
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19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer?
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19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer?.
19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer?.
Solutions for 19g of water at 30oC and 5g of ice at − 20oC are mixed together in a calorimeter. What is the final temperature of the mixture ? Given specific heat of ice = 0.5 cal g− 1(oC)− 1 and latent heat of fusion of ice = 0.8 cal g−1a)0o Cb)− 5o Cc)5o Cd)10o CCorrect answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for NEET.
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