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Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

In a ten litr...

Question

In a ten litre vessel, the total pressure of a gaseous mixture containing $H_{2}, N_{2}$ and $C O_{2}$ is $9.8$ $a t m$ . The partial pressures of $H_{2}$ and $N_{2}$ are $3.7$ and $4.2$ $a t m$ , respectively. The partial pressure of $C O_{2}$ is:

1.9

a t m

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0.19

a t m

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2.4

a t m

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0.019

a t m

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Solution

The correct option is A $1.9$ $a t m$
According to Dalton's law of partial pressure,

$P_{C O_{2}} = P - (P_{H_{2}} + P_{N_{2}})$

$P_{C O_{2}} = 9.8 - (3.7 + 4.2) = 1.9$ $a t m$

Hence, option A is correct.

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Similar questions

In a 10 litre vessel, the total pressure of a gaseous mixture containing $H_{2}, N_{2} a n d C O_{2}$ is 9.8 atm, The partial pressures of $H_{2} a n d N_{2}$ are 3.7 and 4.2 atm respectively. Find the partial pressure of $C O_{2}$ .

Q. 5 litre of

N_{2}

under a pressure of 2 atm, 2 litre of

O_{2}

at 5.5 atm and 3 litre of

C O_{2}

at 5 atm are mixed. The resultant volume of the mixture is 15 litre. Calculate the total pressure of the mixture and partial pressure of each constituent.

Q. For the gaseous reaction

N_{2} + 3 H_{2} ⇌ {2 N H}_{3}

The partial pressure of

H_{2}

and

N_{2}

are 0.4 and 0.8 atm respectively. The total pressure of the entire system is 2.80 atm. The equilibrium constant

K_{p}

will be:

If a mixture of $C O_{2} a n d N_{2}$ in equal amount exert a total pressure of 1 atm, the partial pressure of $N_{2}$ in the mixture is –

Q. For the gaseous reaction

3 H_{2} + N_{2} \Leftrightarrow 2 N H_{3}

, the equilibrium pressures of

H_{2}

and

N_{2}

are

0.4

atm and

0.8

atm respectively. The total pressure of the equilibrium system is

2.8

atm. The value of

K p

is:

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In a ten litre vessel, the total pressure of a gaseous mixture containing H2,N2 and CO2 is 9.8 atm. The partial pressures of H2 and N2 are 3.7 and 4.2 atm, respectively. The partial pressure of CO2 is:

The correct option is A 1.9 atmAccording to Dalton's law of partial pressure,PCO2=P−(PH2+PN2)PCO2=9.8−(3.7+4.2)=1.9 atmHence, option A is correct.

In a ten litre vessel, the total pressure of a gaseous mixture containing $H_{2}, N_{2}$ and $C O_{2}$ is $9.8$ $a t m$ . The partial pressures of $H_{2}$ and $N_{2}$ are $3.7$ and $4.2$ $a t m$ , respectively. The partial pressure of $C O_{2}$ is:

The correct option is A $1.9$ $a t m$
According to Dalton's law of partial pressure,

$P_{C O_{2}} = P - (P_{H_{2}} + P_{N_{2}})$

$P_{C O_{2}} = 9.8 - (3.7 + 4.2) = 1.9$ $a t m$

Hence, option A is correct.