(C) The ideal gas equation is given by $PV = nRT$.Rearranging for concentration $C = \frac{n}{V}$,we get $P = CRT$.Given $P = 1 \, atm$,$C = 1 \, mol

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(C) The ideal gas equation is given by $PV = nRT$.Rearranging for concentration $C = \frac{n}{V}$,we get $P = CRT$.Given $P = 1 \, atm$,$C = 1 \, mol \, L^{-1}$,and $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$.Substituting these values: $1 = 1 \times 0.082 \times T$.Therefore,$T = \frac{1}{0.082} \approx 12.19 \, K$.Thus,the condition is $T \approx 12 \, K$.

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

Medium

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of $1 \, atm$ but also a concentration of $1 \, mol \, L^{-1}$ $(R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1})$?

AIPMT 1993 All AIPMT

A
At $STP$
B
When $V = 22.4 \, L$
C
When $T = 12 \, K$
D
Impossible under any conditions

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Ideal gas equation and Related gas laws

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AIPMT 1993 Paper All AIPMT years →

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Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of $1 \, atm$ but also a concentration of $1 \, mol \, L^{-1}$ $(R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1})$?

Similar Questions

$34.05 \, mL$ of phosphorus vapour weighs $0.0625 \, g$ at $546^{\circ} C$ and $0.1 \, bar$ pressure. What is the molar mass of phosphorus?

For a fixed amount of gas at constant pressure,provide the plot of volume $(V)$ versus temperature $(T)$ in Kelvin. What does it represent?

$A$ mass of gas occupies $11.2 \ dm^3$ at $105 \ kPa$. What is its volume if the pressure is increased to $210 \ kPa$ at constant temperature (in $dm^3$)?

At $273 \, K$ temperature and $1 \, bar$ pressure,if the volume of a gas increases by $20 \%$,what temperature is required assuming pressure remains constant (in $, K$)?

At what temperature does the volume of a gas become theoretically zero?

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