1 mol N2 and 3 mol H2 are introduced in 8.21 litre container initially at 27∘C where no chemical reaction takes place. Select the correct statement(s).

Pressure can be calculated as,P=4×0.0821×3008.21=12atmPN2=14×12, PH2=34×12=3 atm =9 atmAt 600 K = 6 atmN26+3H218⟶2NH3

1 mol N2 and 3 mol H2 are introduced in 8.21 litre container initially at 27∘C where no chemical reaction takes place. Select the correct statement(s).

Pressure can be calculated as,P=4×0.0821×3008.21=12atmPN2=14×12, PH2=34×12=3 atm =9 atmAt 600 K = 6 atmN26+3H218⟶2NH3

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1 mol N₂ and 3 mol H₂are introduced in 8.21 litre container initially at $27^{\circ} C$ where no chemical reaction takes place. Select the correct statement(s).

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Partial pressure of N₂is 12 atn

Partial pressure of N₂ is 3 atm

Total pressure is 9 atm

If temperature is increased to 600 K and NH₃ formation takes place with 100 % yield then total pressure developed is 12 atm

answer is B, D.

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Detailed Solution

Pressure can be calculated as,

$P = \frac{4 \times 0.0821 \times 300}{8.21} = 12 atm$

$P_{N_{2}} = \frac{1}{4} \times 12, P_{H_{2}} = \frac{3}{4} \times 12$

$= 3 atm = 9 atm$

At $600 K = 6 atm$

$\underset{6}{N_{2}} + \underset{18}{3 H_{2}} ⟶ 2 {NH}_{3}$

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1 mol N2 and 3 mol H2 are introduced in 8.21 litre container initially at 27∘C where no chemical reaction takes place. Select the correct statement(s).

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1 mol N₂ and 3 mol H₂are introduced in 8.21 litre container initially at $27^{\circ} C$ where no chemical reaction takes place. Select the correct statement(s).