The pressure exerted by a mixture of 3-5 g of N2 and 4g of H2 contained in a 8-21 dm-3 flask at 27-C is-1- 5-925 atm-2- 6-375 atm-3- 8-217 atm-4- 3-291 atm

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Standard XII

Chemistry

Azeotropic Mixtures

The pressure ...

Question

The pressure exerted by a mixture of 3.5 g of N₂ and 4g of H₂ contained in a 8.21 dm−3 flask at 27°C is
(1) 5.925 atm
(2) 6.375 atm
(3) 8.217 atm
(4) 3.291 atm

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Solution

Step 1:

Given that, the weight of N₂=3.2g
weight of H₂=4g
the volume of the flask = 8.21dm−3=8.21L
temperature = 27+273=300K
Step 2:
Total number of moles = 3.528+42=2.125

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The pressure exerted by a mixture of 3.5 g of N2 and 4g of H2 contained in a 8.21 dm−3 flask at 27°C is(1) 5.925 atm(2) 6.375 atm(3) 8.217 atm(4) 3.291 atm

Step 1: Given that, the weight of N2=3.2g weight of H2=4g the volume of the flask = 8.21dm−3=8.21L temperature = 27+273=300K Step 2: Total number of moles = 3.528+42=2.125

The pressure exerted by a mixture of 3.5 g of N₂ and 4g of H₂ contained in a 8.21 dm−3 flask at 27°C is
(1) 5.925 atm
(2) 6.375 atm
(3) 8.217 atm
(4) 3.291 atm

Step 1:

Given that, the weight of N₂=3.2g
weight of H₂=4g
the volume of the flask = 8.21dm−3=8.21L
temperature = 27+273=300K
Step 2:
Total number of moles = 3.528+42=2.125