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One mole of N2O4 is kept in a close container at 300K and 1 atm pressure. When it is heated to 600 K 20% of it decomposes to NO2 (g). Calculate the resultant pressure exerted on the walls of the container
- a)3.4 atm
- b)2.4 atm
- c)2.0 atm
- d)3.6 atm
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
One mole of N2O4is kept in a close container at 300K and 1 atm pressur...
N2O4 ⇔ 2NO2
1mole 0 Initial moles
-20% of 1=0.2 +2(20% of 1)=0.40 At equilibrium
1-0.2= 0.8 0.4 Moles at equilibrium
Total moles at equilibrium = 0.8+0.4 = 1.2 moles
1 mole vapour pressure = 1 atm at 300 K
Applying PV = nRT
1xV = 1x R x 300 .... (1)
When n=1.2 moles, T = 600 K
P x V = 1.2 x R x 600 .... (2)
Dividing (2) by (1),
PxV/(1xV) = (1.2 x R x 600)/ (1 x R x 300)
Therefore, P= 2.4 atm
Hence, resultant pressure of mixture is 2.4 atm
1mole 0 Initial moles
-20% of 1=0.2 +2(20% of 1)=0.40 At equilibrium
1-0.2= 0.8 0.4 Moles at equilibrium
Total moles at equilibrium = 0.8+0.4 = 1.2 moles
1 mole vapour pressure = 1 atm at 300 K
Applying PV = nRT
1xV = 1x R x 300 .... (1)
When n=1.2 moles, T = 600 K
P x V = 1.2 x R x 600 .... (2)
Dividing (2) by (1),
PxV/(1xV) = (1.2 x R x 600)/ (1 x R x 300)
Therefore, P= 2.4 atm
Hence, resultant pressure of mixture is 2.4 atm
Most Upvoted Answer
One mole of N2O4is kept in a close container at 300K and 1 atm pressur...
To solve this problem, we need to use the ideal gas law equation, which states:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
Given:
Initial conditions: T1 = 300 K, P1 = 1 atm
Final conditions: T2 = 600 K, P2 = ?
Step 1: Determine the number of moles of N2O4
Since we are given that one mole of N2O4 is present initially, the number of moles of N2O4 remains the same throughout the process.
n = 1 mole
Step 2: Calculate the number of moles of NO2 formed
According to the given information, 20% of N2O4 decomposes to NO2(g).
n(NO2) = 0.2 * n(N2O4)
n(NO2) = 0.2 * 1 mole
n(NO2) = 0.2 moles
Step 3: Calculate the number of moles of N2O4 remaining
Since 20% of N2O4 decomposes, the remaining amount is 80% of the initial amount.
n(N2O4 remaining) = 0.8 * n(N2O4)
n(N2O4 remaining) = 0.8 * 1 mole
n(N2O4 remaining) = 0.8 moles
Step 4: Calculate the final pressure
To find the final pressure, we need to consider both the moles of NO2 and the moles of N2O4 remaining.
Total moles of gas = moles of NO2 + moles of N2O4 remaining
Total moles of gas = 0.2 moles + 0.8 moles
Total moles of gas = 1 mole
Using the ideal gas law equation, we can now calculate the final pressure.
P2 * V = n * R * T2
Substituting the values:
P2 * V = 1 mole * R * 600 K
Since the volume is constant, we can simplify the equation to:
P2 = (1 mole * R * 600 K) / V
Step 5: Determine the final pressure in terms of the initial pressure
Since the volume and the number of moles remain constant, we can write the ratio of the final pressure to the initial pressure as:
P2 / P1 = T2 / T1
Substituting the values:
P2 / 1 atm = 600 K / 300 K
Simplifying the equation, we find:
P2 = 2 atm
Therefore, the resultant pressure exerted on the walls of the container is 2 atm, which corresponds to option B.
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
Given:
Initial conditions: T1 = 300 K, P1 = 1 atm
Final conditions: T2 = 600 K, P2 = ?
Step 1: Determine the number of moles of N2O4
Since we are given that one mole of N2O4 is present initially, the number of moles of N2O4 remains the same throughout the process.
n = 1 mole
Step 2: Calculate the number of moles of NO2 formed
According to the given information, 20% of N2O4 decomposes to NO2(g).
n(NO2) = 0.2 * n(N2O4)
n(NO2) = 0.2 * 1 mole
n(NO2) = 0.2 moles
Step 3: Calculate the number of moles of N2O4 remaining
Since 20% of N2O4 decomposes, the remaining amount is 80% of the initial amount.
n(N2O4 remaining) = 0.8 * n(N2O4)
n(N2O4 remaining) = 0.8 * 1 mole
n(N2O4 remaining) = 0.8 moles
Step 4: Calculate the final pressure
To find the final pressure, we need to consider both the moles of NO2 and the moles of N2O4 remaining.
Total moles of gas = moles of NO2 + moles of N2O4 remaining
Total moles of gas = 0.2 moles + 0.8 moles
Total moles of gas = 1 mole
Using the ideal gas law equation, we can now calculate the final pressure.
P2 * V = n * R * T2
Substituting the values:
P2 * V = 1 mole * R * 600 K
Since the volume is constant, we can simplify the equation to:
P2 = (1 mole * R * 600 K) / V
Step 5: Determine the final pressure in terms of the initial pressure
Since the volume and the number of moles remain constant, we can write the ratio of the final pressure to the initial pressure as:
P2 / P1 = T2 / T1
Substituting the values:
P2 / 1 atm = 600 K / 300 K
Simplifying the equation, we find:
P2 = 2 atm
Therefore, the resultant pressure exerted on the walls of the container is 2 atm, which corresponds to option B.
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One mole of N2O4is kept in a close container at 300K and 1 atm pressure. When it is heated to 600 K 20% of it decomposes to NO2(g). Calculate the resultant pressure exerted on the walls of the containera)3.4 atmb)2.4 atmc)2.0 atmd)3.6 atmCorrect answer is option 'B'. Can you explain this answer?
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