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4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50
o
C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?
o
C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?
Most Upvoted Answer
4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a tempe...
To solve this problem, we need to apply the ideal gas law and the concept of molar mass.
First, let's calculate the number of moles of argon gas in the bulb initially.
Given:
Mass of argon gas = 4g
Atomic mass of argon (Ar) = 40g/mol
Using the formula:
Number of moles = Mass / Molar mass
Number of moles of argon gas = 4g / 40g/mol = 0.1 mol
Now, let's calculate the pressure of the gas in the bulb initially.
Given:
Temperature = TK
Pressure = P atm
Using the ideal gas law:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
Since we are only interested in the temperature, let's rearrange the equation as follows:
T = PV / (nR)
Now, let's calculate the pressure in terms of moles and volume.
Given:
Pressure = P atm
Using the formula:
Pressure = Force / Area
Force = Mass x Acceleration
Acceleration due to gravity = 9.8 m/s^2
The mass is given as 4g, and the area can be calculated using the volume of the bulb.
Now, let's consider the change in temperature.
Given:
Change in temperature = 50 o C
To find the final temperature, we need to subtract the change in temperature from the initial temperature.
Now, let's calculate the number of moles of argon gas after removing 0.8g.
Given:
Mass of argon gas removed = 0.8g
Using the formula:
Number of moles = Mass / Molar mass
Number of moles of argon gas removed = 0.8g / 40g/mol = 0.02 mol
Now, let's calculate the final pressure of the gas in the bulb.
To get the original pressure, we need to add the 0.02 mol of argon gas back into the bulb and then calculate the pressure.
Finally, let's substitute the values into the rearranged ideal gas law equation and solve for T.
First, let's calculate the number of moles of argon gas in the bulb initially.
Given:
Mass of argon gas = 4g
Atomic mass of argon (Ar) = 40g/mol
Using the formula:
Number of moles = Mass / Molar mass
Number of moles of argon gas = 4g / 40g/mol = 0.1 mol
Now, let's calculate the pressure of the gas in the bulb initially.
Given:
Temperature = TK
Pressure = P atm
Using the ideal gas law:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
Since we are only interested in the temperature, let's rearrange the equation as follows:
T = PV / (nR)
Now, let's calculate the pressure in terms of moles and volume.
Given:
Pressure = P atm
Using the formula:
Pressure = Force / Area
Force = Mass x Acceleration
Acceleration due to gravity = 9.8 m/s^2
The mass is given as 4g, and the area can be calculated using the volume of the bulb.
Now, let's consider the change in temperature.
Given:
Change in temperature = 50 o C
To find the final temperature, we need to subtract the change in temperature from the initial temperature.
Now, let's calculate the number of moles of argon gas after removing 0.8g.
Given:
Mass of argon gas removed = 0.8g
Using the formula:
Number of moles = Mass / Molar mass
Number of moles of argon gas removed = 0.8g / 40g/mol = 0.02 mol
Now, let's calculate the final pressure of the gas in the bulb.
To get the original pressure, we need to add the 0.02 mol of argon gas back into the bulb and then calculate the pressure.
Finally, let's substitute the values into the rearranged ideal gas law equation and solve for T.
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4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?
Question Description
4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?.
4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?.
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4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :?, a detailed solution for 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? has been provided alongside types of 4g argon in a bulb at a g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in hot bath at a temperature 50 o C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :? theory, EduRev gives you an
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