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56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:
- a)4, 6
- b)5, 5
- c)6, 4
- d)2, 8
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a to...
Raoult's Law states that the partial vapour pressure of a component in a mixture is equal to the vapour pressure of the pure component at that temperature multiplied by its mole fraction in the mixture.
In a mixture of liquids of A and B,
pA=xA×p
pB=xB×p
moles of nitrogen gas is nN2=56/28=2 mol
moles of oxygen gas is nO2=96/32=3 mol
Mole fraction of nitrogen is xN2=2/(2+3)=0.4
Mole fraction of oxygen will be xO2=1−0.4=0.6
Partial pressure of oxygen is pO2=0.6×10=6 atm
Partial pressure of Nitrogen is pN2=0.4×10=4 atm
Most Upvoted Answer
56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a to...
Given:
Mass of nitrogen (N2) = 56 g
Mass of oxygen (O2) = 96 g
Total pressure = 10 atm
To find:
Partial pressures of oxygen and nitrogen
Formula to calculate partial pressure:
Partial pressure = (Mole fraction of the component) x (Total pressure)
Step 1: Calculate the moles of nitrogen and oxygen
Moles of nitrogen (N2) = Mass of nitrogen / Molar mass of nitrogen
Molar mass of nitrogen (N2) = 2 x atomic mass of nitrogen (N) = 2 x 14 = 28 g/mol
Moles of nitrogen (N2) = 56 g / 28 g/mol = 2 mol
Moles of oxygen (O2) = Mass of oxygen / Molar mass of oxygen
Molar mass of oxygen (O2) = 2 x atomic mass of oxygen (O) = 2 x 16 = 32 g/mol
Moles of oxygen (O2) = 96 g / 32 g/mol = 3 mol
Step 2: Calculate the mole fraction of nitrogen and oxygen
Mole fraction of nitrogen (XN2) = Moles of nitrogen / Total moles of gas
Total moles of gas = Moles of nitrogen + Moles of oxygen = 2 mol + 3 mol = 5 mol
Mole fraction of nitrogen (XN2) = 2 mol / 5 mol = 0.4
Mole fraction of oxygen (XO2) = Moles of oxygen / Total moles of gas
Mole fraction of oxygen (XO2) = 3 mol / 5 mol = 0.6
Step 3: Calculate the partial pressures of nitrogen and oxygen
Partial pressure of nitrogen (PN2) = Mole fraction of nitrogen (XN2) x Total pressure
Partial pressure of nitrogen (PN2) = 0.4 x 10 atm = 4 atm
Partial pressure of oxygen (PO2) = Mole fraction of oxygen (XO2) x Total pressure
Partial pressure of oxygen (PO2) = 0.6 x 10 atm = 6 atm
Therefore, the partial pressures of oxygen and nitrogen are 6 atm and 4 atm respectively. Hence, the correct answer is option C.
Mass of nitrogen (N2) = 56 g
Mass of oxygen (O2) = 96 g
Total pressure = 10 atm
To find:
Partial pressures of oxygen and nitrogen
Formula to calculate partial pressure:
Partial pressure = (Mole fraction of the component) x (Total pressure)
Step 1: Calculate the moles of nitrogen and oxygen
Moles of nitrogen (N2) = Mass of nitrogen / Molar mass of nitrogen
Molar mass of nitrogen (N2) = 2 x atomic mass of nitrogen (N) = 2 x 14 = 28 g/mol
Moles of nitrogen (N2) = 56 g / 28 g/mol = 2 mol
Moles of oxygen (O2) = Mass of oxygen / Molar mass of oxygen
Molar mass of oxygen (O2) = 2 x atomic mass of oxygen (O) = 2 x 16 = 32 g/mol
Moles of oxygen (O2) = 96 g / 32 g/mol = 3 mol
Step 2: Calculate the mole fraction of nitrogen and oxygen
Mole fraction of nitrogen (XN2) = Moles of nitrogen / Total moles of gas
Total moles of gas = Moles of nitrogen + Moles of oxygen = 2 mol + 3 mol = 5 mol
Mole fraction of nitrogen (XN2) = 2 mol / 5 mol = 0.4
Mole fraction of oxygen (XO2) = Moles of oxygen / Total moles of gas
Mole fraction of oxygen (XO2) = 3 mol / 5 mol = 0.6
Step 3: Calculate the partial pressures of nitrogen and oxygen
Partial pressure of nitrogen (PN2) = Mole fraction of nitrogen (XN2) x Total pressure
Partial pressure of nitrogen (PN2) = 0.4 x 10 atm = 4 atm
Partial pressure of oxygen (PO2) = Mole fraction of oxygen (XO2) x Total pressure
Partial pressure of oxygen (PO2) = 0.6 x 10 atm = 6 atm
Therefore, the partial pressures of oxygen and nitrogen are 6 atm and 4 atm respectively. Hence, the correct answer is option C.
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56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer?
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56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about 56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer?.
56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about 56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:a)4, 6b)5, 5c)6, 4d)2, 8Correct answer is option 'C'. Can you explain this answer?.
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