Which of the following gases of the same mass | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) Let the mass of each gas be $m = 1 \ g$. The number of moles $n = \frac{m}{M}$,where $M$ is the molar mass. Since $m$ is constant,$n \propto \frac

Vedclass · Accepted Answer

$H_2$

Vedclass · Answer

(A) Let the mass of each gas be $m = 1 \ g$. The number of moles $n = \frac{m}{M}$,where $M$ is the molar mass. Since $m$ is constant,$n \propto \frac{1}{M}$. The molar masses are: $M(H_2) = 2 \ g/mol$,$M(N_2) = 28 \ g/mol$,$M(O_2) = 32 \ g/mol$,$M(Cl_2) = 71 \ g/mol$. Thus,the number of moles follows the order: $n(H_2) > n(N_2) > n(O_2) > n(Cl_2)$. From the ideal gas equation $PV = nRT$,at constant $T$ and $V$,$P \propto n$. Therefore,the gas with the highest number of moles will exert the highest pressure. Since $H_2$ has the lowest molar mass,it has the highest number of moles for a given mass,and thus exerts the highest pressure.

Which of the following gases of the same mass exerts the highest pressure at a constant temperature?

Similar Questions

Calculate the density of a gaseous mixture which consists of $3.01 \times 10^{24}$ molecules of $N_2$ and $32 \ g$ of $O_2$ gas at $3 \ atm$ pressure and $860 \ K$ temperature. (Given: $R = 1/12 \ atm \ L \ mol^{-1} \ K^{-1}$) ............. $g/L$

$A$ vessel of $120 \, mL$ capacity contains a certain amount of gas at $35^{\circ} C$ and $1.2 \, bar$ pressure. The gas is transferred to another vessel of volume $180 \, mL$ at $35^{\circ} C$. What would be its pressure?

At a given temperature,the density of gas $x$ is twice the density of gas $y$. If the molar mass of $y$ is three times the molar mass of $x$,find the ratio of their pressures $(P_x/P_y)$.

At what pressure will a quantity of gas occupy a volume of $60 \, mL$,if it occupies a volume of $100 \, mL$ at a pressure of $720 \, mm$ (assuming temperature is constant)?

Vedclass Test Series

Exam Paper Generator

Online Exam Module