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Number of collisions of molecules of a gas on the wall of a container per m2 will :
- a)Increase if temperature and volume both are doubled.
- b)Increase if temperature and volume both are halved.
- c)Increase if pressure and temperature both are doubled.
- d)Increase if pressure and temperature both are halved.
Correct answer is option 'B,C'. Can you explain this answer?
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Number of collisions of molecules of a gas on the wall of a container ...
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Number of collisions of molecules of a gas on the wall of a container ...
Number of collisions of molecules of a gas on the wall of a container per m2 will increase if:
a) Temperature and volume both are doubled:
When the temperature and volume of a gas both double, the average kinetic energy of the gas molecules also doubles. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the temperature. As the kinetic energy increases, the gas molecules move faster and collide with the walls of the container more frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will increase.
b) Temperature and volume both are halved:
When the temperature and volume of a gas both halve, the average kinetic energy of the gas molecules also halves. As a result, the gas molecules move slower and collide with the walls of the container less frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will decrease.
c) Pressure and temperature both are doubled:
According to the ideal gas law, pressure is directly proportional to the temperature and the number of gas molecules. When both pressure and temperature are doubled, the number of gas molecules remains constant. However, the increase in temperature leads to an increase in the average kinetic energy of the gas molecules. As a result, the gas molecules move faster and collide with the walls of the container more frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will increase.
d) Pressure and temperature both are halved:
Similarly, when both pressure and temperature are halved, the number of gas molecules remains constant. However, the decrease in temperature leads to a decrease in the average kinetic energy of the gas molecules. As a result, the gas molecules move slower and collide with the walls of the container less frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will decrease.
In summary, the number of collisions of molecules on the wall of a container per unit area is directly influenced by the temperature, volume, and pressure of the gas. When temperature and volume are doubled or halved, or when pressure and temperature are doubled or halved, the number of collisions will increase or decrease accordingly.
a) Temperature and volume both are doubled:
When the temperature and volume of a gas both double, the average kinetic energy of the gas molecules also doubles. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the temperature. As the kinetic energy increases, the gas molecules move faster and collide with the walls of the container more frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will increase.
b) Temperature and volume both are halved:
When the temperature and volume of a gas both halve, the average kinetic energy of the gas molecules also halves. As a result, the gas molecules move slower and collide with the walls of the container less frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will decrease.
c) Pressure and temperature both are doubled:
According to the ideal gas law, pressure is directly proportional to the temperature and the number of gas molecules. When both pressure and temperature are doubled, the number of gas molecules remains constant. However, the increase in temperature leads to an increase in the average kinetic energy of the gas molecules. As a result, the gas molecules move faster and collide with the walls of the container more frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will increase.
d) Pressure and temperature both are halved:
Similarly, when both pressure and temperature are halved, the number of gas molecules remains constant. However, the decrease in temperature leads to a decrease in the average kinetic energy of the gas molecules. As a result, the gas molecules move slower and collide with the walls of the container less frequently. Therefore, the number of collisions of molecules on the wall of the container per unit area will decrease.
In summary, the number of collisions of molecules on the wall of a container per unit area is directly influenced by the temperature, volume, and pressure of the gas. When temperature and volume are doubled or halved, or when pressure and temperature are doubled or halved, the number of collisions will increase or decrease accordingly.
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Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer?
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Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. 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 Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer?.
Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. 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 Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer?.
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Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer?, a detailed solution for Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer? has been provided alongside types of Number of collisions of molecules of a gas on the wall of a container per m2 will :a)Increase if temperature and volume both are doubled.b)Increase if temperature and volume both are halved.c)Increase if pressure and temperature both are doubled.d)Increase if pressure and temperature both are halved.Correct answer is option 'B,C'. Can you explain this answer? theory, EduRev gives you an
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