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Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)
- a)62 J
- b)104 J
- c)124 J
- d)208 J
Correct answer is option 'D'. Can you explain this answer?
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Two moles of ideal helium gas are in a rubber balloon at 30°C. The...
The heat is supplied at constant pressure.
Therefore
Therefore
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Two moles of ideal helium gas are in a rubber balloon at 30°C. The...
°C. The balloon is then heated to 70°C. Assuming the volume of the balloon remains constant, calculate the final pressure of the helium gas.
To solve this problem, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature (in Kelvin)
First, let's convert the initial and final temperatures to Kelvin:
Initial temperature = 30°C = 30 + 273 = 303 K
Final temperature = 70°C = 70 + 273 = 343 K
Since the volume of the balloon remains constant, we can cancel it out from the equation. Therefore, we have:
P1/T1 = P2/T2
Where:
P1 = initial pressure
T1 = initial temperature
P2 = final pressure
T2 = final temperature
Substituting the values into the equation:
P1/303 = P2/343
Now, we can solve for P2:
P2 = (P1 * T2) / T1
Given that P1 is not provided in the question, we cannot determine the final pressure without this information.
To solve this problem, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature (in Kelvin)
First, let's convert the initial and final temperatures to Kelvin:
Initial temperature = 30°C = 30 + 273 = 303 K
Final temperature = 70°C = 70 + 273 = 343 K
Since the volume of the balloon remains constant, we can cancel it out from the equation. Therefore, we have:
P1/T1 = P2/T2
Where:
P1 = initial pressure
T1 = initial temperature
P2 = final pressure
T2 = final temperature
Substituting the values into the equation:
P1/303 = P2/343
Now, we can solve for P2:
P2 = (P1 * T2) / T1
Given that P1 is not provided in the question, we cannot determine the final pressure without this information.
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Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer?
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Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. 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 Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer?.
Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. 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 Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer?.
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Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer?, a detailed solution for Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer? has been provided alongside types of Two moles of ideal helium gas are in a rubber balloon at 30°C. The balloon is fully expandable and can be assumed to require no energy in its expansion. The temperature of the gas in the balloon is slowly changed to 35°C. The amount of heat required in raising the temperature is nearly (take R = 8.31 J/mol.K)a)62 Jb)104 Jc)124 Jd)208 JCorrect answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
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