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A gaseous mixture was prepared by taking equal mole of CO and N2. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen (N2) in the mixture is :
- a)0.5 atm
- b)0.8 atm [2011]
- c)0.9 atm
- d)1 atm
Correct answer is option 'A'. Can you explain this answer?
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A gaseous mixture was prepared by taking equal mole of CO and N2. If t...
Given nCO = nN2 PCO + PN2 = 1 atm
Partial pressure of a gas = mole fraction of gas × total pressure
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A gaseous mixture was prepared by taking equal mole of CO and N2. If t...
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A gaseous mixture was prepared by taking equal mole of CO and N2. If t...
Given:
- Equal moles of CO and N2 are taken to prepare the mixture.
- Total pressure of the mixture is 1 atmosphere.
To find:
The partial pressure of nitrogen (N2) in the mixture.
Solution:
The total pressure of a gaseous mixture is the sum of the partial pressures of each component present in the mixture. Since equal moles of CO and N2 are taken, the mole fraction of each component is 0.5.
We can use Dalton's law of partial pressures to find the partial pressure of nitrogen (N2) in the mixture.
Dalton's Law of Partial Pressures:
According to Dalton's law of partial pressures, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.
Mathematically,
Total pressure (P_total) = Partial pressure of gas A (P_A) + Partial pressure of gas B (P_B) + ...
In this case, we have CO and N2 in the mixture. Therefore,
P_total = P_CO + P_N2
Since equal moles of CO and N2 are taken, the partial pressure of CO (P_CO) is also equal to the partial pressure of N2 (P_N2).
Let's assume the partial pressure of nitrogen (N2) in the mixture is P_N2.
Therefore,
P_total = P_CO + P_N2
1 atm = P_N2 + P_N2
1 atm = 2P_N2
Dividing both sides of the equation by 2, we get:
P_N2 = 1 atm / 2
P_N2 = 0.5 atm
Conclusion:
The partial pressure of nitrogen (N2) in the mixture is 0.5 atm. Therefore, the correct answer is option 'A'.
- Equal moles of CO and N2 are taken to prepare the mixture.
- Total pressure of the mixture is 1 atmosphere.
To find:
The partial pressure of nitrogen (N2) in the mixture.
Solution:
The total pressure of a gaseous mixture is the sum of the partial pressures of each component present in the mixture. Since equal moles of CO and N2 are taken, the mole fraction of each component is 0.5.
We can use Dalton's law of partial pressures to find the partial pressure of nitrogen (N2) in the mixture.
Dalton's Law of Partial Pressures:
According to Dalton's law of partial pressures, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.
Mathematically,
Total pressure (P_total) = Partial pressure of gas A (P_A) + Partial pressure of gas B (P_B) + ...
In this case, we have CO and N2 in the mixture. Therefore,
P_total = P_CO + P_N2
Since equal moles of CO and N2 are taken, the partial pressure of CO (P_CO) is also equal to the partial pressure of N2 (P_N2).
Let's assume the partial pressure of nitrogen (N2) in the mixture is P_N2.
Therefore,
P_total = P_CO + P_N2
1 atm = P_N2 + P_N2
1 atm = 2P_N2
Dividing both sides of the equation by 2, we get:
P_N2 = 1 atm / 2
P_N2 = 0.5 atm
Conclusion:
The partial pressure of nitrogen (N2) in the mixture is 0.5 atm. Therefore, the correct answer is option 'A'.
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A gaseous mixture was prepared by taking equal mole of CO and N2. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen (N2) in the mixture is :a)0.5 atmb)0.8 atm [2011]c)0.9 atmd)1 atmCorrect answer is option 'A'. Can you explain this answer?
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