(A) The ideal gas equation is $PV = nRT$,which gives $R = \frac{PV}{nT}$.At $STP$,for $1 \, mol$ of an ideal gas,the pressure $P = 1 \, atm$,volume $V

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$0.082 \, L \, atm \, K^{-1} \, mol^{-1}$

(A) The ideal gas equation is $PV = nRT$,which gives $R = \frac{PV}{nT}$.At $STP$,for $1 \, mol$ of an ideal gas,the pressure $P = 1 \, atm$,volume $V = 22.4 \, L$,and temperature $T = 273.15 \, K$.Substituting these values: $R = \frac{1 \, atm \times 22.4 \, L}{1 \, mol \times 273.15 \, K} \approx 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$.

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

Medium

The value of the gas constant $R$ is closest to which of the following values?

A
$0.082 \, L \, atm \, K^{-1} \, mol^{-1}$
B
$0.082 \, L \, atm^{-1} \, mol$
C
$0.082 \, L \, atm \, K$
D
$0.082 \, L \, atm^{-1} \, K \, mol^{-1}$

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Ideal gas equation and Related gas laws

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The value of the gas constant $R$ is closest to which of the following values?

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$A$ vessel of volume $24.6 \ L$ contains $1.5 \ moles$ of $H_2$ and $2.5 \ moles$ of $N_2$ at $300 \ K$. Calculate the partial pressure of $N_2$ in the vessel. (in $atm$)

The pressure of an $LPG$ gas cylinder is $14.9 \ bar$,which is considered safe. If the pressure is $12 \ bar$ at $27 \ ^oC$,at what temperature will the cylinder blast (in $K$)?

In an experiment during the analysis of a carbon compound,$145 \ L$ of $H_2$ was collected at $760 \ mm \ Hg$ pressure and $27 \ ^oC$ temperature. The mass of $H_2$ is nearly $....... \ g$.

If the density ratio of a gas is $1:2$ and the temperature ratio is $2:1$,what will be the ratio of their pressures?

If the density of gas $A$ is $1.5$ times that of gas $B$,and the molecular mass of $A$ is $M$,then the molecular mass of $B$ is:

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