(D) Using the ideal gas equation: $PV = nRT$Given: $P = 200 \, Pa$,$V = 10 \, m^3$,$T = 1000 \, K$,$n = (0.5 + x) \, mol$.Substituting the values: $20

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(D) Using the ideal gas equation: $PV = nRT$Given: $P = 200 \, Pa$,$V = 10 \, m^3$,$T = 1000 \, K$,$n = (0.5 + x) \, mol$.Substituting the values: $200 \times 10 = (0.5 + x) \times R \times 1000$$2000 = (0.5 + x) \times 1000R$$2 = (0.5 + x)R$$\frac{2}{R} = 0.5 + x$$x = \frac{2}{R} - 0.5$$x = \frac{2 - 0.5R}{R} = \frac{4 - R}{2R}$

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

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$0.5 \, mol$ of gas $A$ and $x \, mol$ of gas $B$ exert a pressure of $200 \, Pa$ in a container of volume $10 \, m^3$ at $1000 \, K$. Given $R$ is the gas constant in $J \, K^{-1} \, mol^{-1}$,$x$ is

JEE MAIN 2019 All JEE MAIN

A
$\frac{2R}{4 + R}$
B
$\frac{2R}{4 - R}$
C
$\frac{4 + R}{2R}$
D
$\frac{4 - R}{2R}$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

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What is the density of $SO_2$ gas at $27\,^oC$ temperature and $2\, atm$ pressure in $g/L$? (Atomic weights: $S = 32, O = 16, R = 0.082\, L\, atm\, K^{-1}\, mol^{-1}$)

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At $127 \, ^oC$ temperature,the volume of a gas is $3 \, L$. If the volume of the gas becomes half at constant pressure,calculate the final temperature in Kelvin. (in $, K$)

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The density of gas $A$ is twice that of gas $B$ at the same temperature. The molecular weight of gas $B$ is twice that of gas $A$. The ratio of the pressure of gas $A$ to gas $B$ will be:

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If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be:

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The density of $O_{2(g)}$ is maximum at?

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$0.5 \, mol$ of gas $A$ and $x \, mol$ of gas $B$ exert a pressure of $200 \, Pa$ in a container of volume $10 \, m^3$ at $1000 \, K$. Given $R$ is the gas constant in $J \, K^{-1} \, mol^{-1}$,$x$ is

Similar Questions

What is the density of $SO_2$ gas at $27\,^oC$ temperature and $2\, atm$ pressure in $g/L$? (Atomic weights: $S = 32, O = 16, R = 0.082\, L\, atm\, K^{-1}\, mol^{-1}$)

At $127 \, ^oC$ temperature,the volume of a gas is $3 \, L$. If the volume of the gas becomes half at constant pressure,calculate the final temperature in Kelvin. (in $, K$)

The density of gas $A$ is twice that of gas $B$ at the same temperature. The molecular weight of gas $B$ is twice that of gas $A$. The ratio of the pressure of gas $A$ to gas $B$ will be:

If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be:

The density of $O_{2(g)}$ is maximum at?

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