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A vessel contains 0.16g of methane and 0.28g of nitrogen. The ratio of partial pressures of methane to nitrogen in the mixture is about:
- a)7 : 4
- b)1 : 1
- c)4 : 7
- d)2 : 3
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
A vessel contains 0.16g of methane and 0.28g of nitrogen. The ratio of...
We know, Partial pressure of a gas = mole fraction of that gas x Total pressure of mixture of the gases.
Using this formula and using the information given in this question, we get
ratio of partial pressures of methane to nitrogen in the mixture as: 1:1Free Test
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A vessel contains 0.16g of methane and 0.28g of nitrogen. The ratio of...
To find the ratio of partial pressures of methane to nitrogen in the mixture, we need to first calculate the moles of methane and nitrogen present in the vessel.
Step 1: Calculate the moles of methane.
Given: Mass of methane = 0.16g, Molar mass of methane (CH4) = 16g/mol.
Number of moles of methane = Mass of methane / Molar mass of methane
= 0.16g / 16g/mol
= 0.01 mol
Step 2: Calculate the moles of nitrogen.
Given: Mass of nitrogen = 0.28g, Molar mass of nitrogen (N2) = 28g/mol.
Number of moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen
= 0.28g / 28g/mol
= 0.01 mol
Step 3: Calculate the partial pressures of methane and nitrogen.
Partial pressure is directly proportional to the number of moles of a gas.
Partial pressure of methane = Number of moles of methane * Total pressure
= 0.01 mol * Total pressure
Partial pressure of nitrogen = Number of moles of nitrogen * Total pressure
= 0.01 mol * Total pressure
Step 4: Simplify the ratio of partial pressures.
To find the ratio of partial pressures, we can cancel out the common factor of Total pressure.
Ratio of partial pressures of methane to nitrogen = (0.01 mol * Total pressure) / (0.01 mol * Total pressure)
= 1:1
Therefore, the correct answer is option B, 1:1. The ratio of partial pressures of methane to nitrogen in the mixture is 1:1.
Step 1: Calculate the moles of methane.
Given: Mass of methane = 0.16g, Molar mass of methane (CH4) = 16g/mol.
Number of moles of methane = Mass of methane / Molar mass of methane
= 0.16g / 16g/mol
= 0.01 mol
Step 2: Calculate the moles of nitrogen.
Given: Mass of nitrogen = 0.28g, Molar mass of nitrogen (N2) = 28g/mol.
Number of moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen
= 0.28g / 28g/mol
= 0.01 mol
Step 3: Calculate the partial pressures of methane and nitrogen.
Partial pressure is directly proportional to the number of moles of a gas.
Partial pressure of methane = Number of moles of methane * Total pressure
= 0.01 mol * Total pressure
Partial pressure of nitrogen = Number of moles of nitrogen * Total pressure
= 0.01 mol * Total pressure
Step 4: Simplify the ratio of partial pressures.
To find the ratio of partial pressures, we can cancel out the common factor of Total pressure.
Ratio of partial pressures of methane to nitrogen = (0.01 mol * Total pressure) / (0.01 mol * Total pressure)
= 1:1
Therefore, the correct answer is option B, 1:1. The ratio of partial pressures of methane to nitrogen in the mixture is 1:1.
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