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One mole of N2O4(g) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is:
- a)1.2 atm
- b)2.4 atm
- c)2.0 atm
- d)1.0 atm
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
One mole of N2O4(g) at 300 K is kept in a closed container under one a...
N2O4 → 2NO2
moles of unreacted N2O4 = 1 (1 - 0.2) = 0.8
moles of NO2 = 2 * 0.2 = 0.4
- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - (+)
total moles n2 = 0.8 + 0.4 = 1.2
P1/(T1 n1) = P2/(T2 * n2)
1/(300 * 1) = P2/(600 * 1.2)
P2 = 2.4 atm
moles of unreacted N2O4 = 1 (1 - 0.2) = 0.8
moles of NO2 = 2 * 0.2 = 0.4
- - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - - (+)
total moles n2 = 0.8 + 0.4 = 1.2
P1/(T1 n1) = P2/(T2 * n2)
1/(300 * 1) = P2/(600 * 1.2)
P2 = 2.4 atm
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One mole of N2O4(g) at 300 K is kept in a closed container under one a...
Given:
- One mole of N2O4(g) at 300 K
- Closed container under one atmosphere pressure
- Heated to 600 K
- 20% by mass of N2O4(g) decomposes to NO2(g)
To find:
Resultant pressure
Solution:
Step 1: Calculate the initial number of moles of N2O4(g)
We are given that we have one mole of N2O4(g). So the initial number of moles of N2O4(g) is 1.
Step 2: Calculate the final number of moles of N2O4(g) and NO2(g)
Since 20% by mass of N2O4(g) decomposes, only 80% remains. This means that 80% of one mole of N2O4(g) remains, which is 0.8 moles of N2O4(g).
Since the reaction is as follows:
N2O4(g) ⇌ 2NO2(g)
For every 1 mole of N2O4(g) that decomposes, 2 moles of NO2(g) are produced. Therefore, the number of moles of NO2(g) produced is twice the number of moles of N2O4(g) that decomposed.
So, the number of moles of NO2(g) produced is 2 * 0.2 = 0.4 moles.
The total number of moles of gas in the container is the sum of the moles of N2O4(g) and NO2(g), which is 0.8 + 0.4 = 1.2 moles.
Step 3: Apply the Ideal Gas Law
The Ideal Gas Law is given by the equation:
PV = nRT
Where:
P is the pressure of the gas
V is the volume of the gas (which is constant in this case)
n is the number of moles of gas
R is the ideal gas constant
T is the temperature in Kelvin
Since the volume is constant and the number of moles and temperature have changed, we can rewrite the equation as:
P1/T1 = P2/T2
Where:
P1 is the initial pressure
T1 is the initial temperature
P2 is the final pressure
T2 is the final temperature
Step 4: Substitute the values into the equation
We are given that the initial pressure is one atmosphere and the initial temperature is 300 K.
Substituting these values into the equation, we get:
1/300 = P2/600
Simplifying the equation, we find:
P2 = 2 atm
So, the resultant pressure is 2 atm.
Therefore, the correct answer is option 'B', 2.4 atm.
- One mole of N2O4(g) at 300 K
- Closed container under one atmosphere pressure
- Heated to 600 K
- 20% by mass of N2O4(g) decomposes to NO2(g)
To find:
Resultant pressure
Solution:
Step 1: Calculate the initial number of moles of N2O4(g)
We are given that we have one mole of N2O4(g). So the initial number of moles of N2O4(g) is 1.
Step 2: Calculate the final number of moles of N2O4(g) and NO2(g)
Since 20% by mass of N2O4(g) decomposes, only 80% remains. This means that 80% of one mole of N2O4(g) remains, which is 0.8 moles of N2O4(g).
Since the reaction is as follows:
N2O4(g) ⇌ 2NO2(g)
For every 1 mole of N2O4(g) that decomposes, 2 moles of NO2(g) are produced. Therefore, the number of moles of NO2(g) produced is twice the number of moles of N2O4(g) that decomposed.
So, the number of moles of NO2(g) produced is 2 * 0.2 = 0.4 moles.
The total number of moles of gas in the container is the sum of the moles of N2O4(g) and NO2(g), which is 0.8 + 0.4 = 1.2 moles.
Step 3: Apply the Ideal Gas Law
The Ideal Gas Law is given by the equation:
PV = nRT
Where:
P is the pressure of the gas
V is the volume of the gas (which is constant in this case)
n is the number of moles of gas
R is the ideal gas constant
T is the temperature in Kelvin
Since the volume is constant and the number of moles and temperature have changed, we can rewrite the equation as:
P1/T1 = P2/T2
Where:
P1 is the initial pressure
T1 is the initial temperature
P2 is the final pressure
T2 is the final temperature
Step 4: Substitute the values into the equation
We are given that the initial pressure is one atmosphere and the initial temperature is 300 K.
Substituting these values into the equation, we get:
1/300 = P2/600
Simplifying the equation, we find:
P2 = 2 atm
So, the resultant pressure is 2 atm.
Therefore, the correct answer is option 'B', 2.4 atm.
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One mole of N2O4(g) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is:a)1.2 atmb)2.4 atmc)2.0 atmd)1.0 atmCorrect answer is option 'B'. Can you explain this answer?
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