a mixture contains 64 g dioxygen and 60 g of neon at atotal pressure of 10 bar the partial pressure in bar of dioxygen and neon are respective
a 4 and 6
b 6 and 4
c 5 and 5
d 8 and 2
Answers
GIVEN :
- Mass of Dioxygen = 64g
- Mass of neon = 60g
- Total Pressure = 10 bar
To find :
Partial pressure in bar of
- Dioxygen
- Neon
Law used :
Here , we will use Dalton's law of partial pressure, which state that total Pressure exerted my mixture of gas ( which do not undergo chemical reaction ) is given by sum of pressure exerted by each gas when kept in container alone ( that is sum of partial pressure of different gas)
Here,
Total Pressure = Partial pressure of Dioxygen + Partial pressure of neon
Also Partial pressure of Dioxygen = Total pressure × mole fraction of Dioxygen
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SOLUTION :
Firstly we need to find mole fraction.
- Number of mole of Dioxygen = 64 ÷ 32
➝ Number of mole of Dioxygen = 2 mol
- Number of mole of Neon = 60 ÷ 20
➝ Number of mole of neon = 3
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- Mole fraction of Dioxygen = Mole of Dioxygen ÷ Total number of mole of gases
➝ Mole fraction of Dioxygen = 2 ÷ (2+3)
➝ Mole fraction of Dioxygen = 2÷5
➝ Mole fraction of Dioxygen = 0.4
- Mole fraction of Neon = Mole of Neon ÷ Total number of mole of gases
➝ Mole fraction of Neon = 3 ÷ (2+3)
➝ Mole fraction of Neon = 3/5
➝ Mole fraction of Neon = 0.6
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Therefore,
- Partial pressure of Dioxygen = 10 × 0.4
➝ Partial pressure of Dioxygen = 4 bar
- Partial pressure of Neon = 10 × 0.6
➝ Partial pressure of Neon = 6 bar
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ANSWER :
Option a) 4 and 6
Answer:
GIVEN :
Mass of Dioxygen = 64g
Mass of neon = 60g
Total Pressure = 10 bar
To find :
Partial pressure in bar of
Dioxygen
Neon
Law used :
Here , we will use Dalton's law of partial pressure, which state that total Pressure exerted my mixture of gas ( which do not undergo chemical reaction ) is given by sum of pressure exerted by each gas when kept in container alone ( that is sum of partial pressure of different gas)
Here,
Total Pressure = Partial pressure of Dioxygen + Partial pressure of neon
Also Partial pressure of Dioxygen = Total pressure × mole fraction of Dioxygen
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SOLUTION :
Firstly we need to find mole fraction.
Number of mole of Dioxygen = 64 ÷ 32
➝ Number of mole of Dioxygen = 2 mol
Number of mole of Neon = 60 ÷ 20
➝ Number of mole of neon = 3
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Mole fraction of Dioxygen = Mole of Dioxygen ÷ Total number of mole of gases
➝ Mole fraction of Dioxygen = 2 ÷ (2+3)
➝ Mole fraction of Dioxygen = 2÷5
➝ Mole fraction of Dioxygen = 0.4
Mole fraction of Neon = Mole of Neon ÷ Total number of mole of gases
➝ Mole fraction of Neon = 3 ÷ (2+3)
➝ Mole fraction of Neon = 3/5
➝ Mole fraction of Neon = 0.6
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Therefore,
Partial pressure of Dioxygen = 10 × 0.4
➝ Partial pressure of Dioxygen = 4 bar
Partial pressure of Neon = 10 × 0.6
➝ Partial pressure of Neon = 6 bar
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ANSWER :
Option a) 4 and 6