Question
Pressure of $1 \mathrm{~g}$ ideal gas $X$ at $300 \mathrm{~K}$ is $2 \mathrm{~atm}$. When $2 \mathrm{~g}$ of another gas $Y$ is introduced in the same vessel at same temperature, the pressure become 3 atm then correct relationship between molar mass of $X$ and $Y$ is :(a) $M_{Y}=2 M_{X}$(b) $M_{Y}=4 M_{X}$(c) $M_{X}=4 M_{Y}$(d). None of these
Step 1
We know that the ideal gas equation is $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles, $R$ is the gas constant, and $T$ is the temperature. Show more…
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Key Concepts
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Pressure of $1 \mathrm{~g}$ of an ideal gas $\mathrm{A}$ at $27^{\circ} \mathrm{C}$ is found to be 2 bar. When $2 \mathrm{~g}$ of another ideal gas $\mathrm{B}$ is introduced in the same flask at same temperature the pressure becomes 3 bar. What is the relationship between their molecular masses? (a) $2 M_{\mathrm{B}}=M_{\mathrm{A}}$ (b) $M_{\mathrm{B}}=M_{\mathrm{A}}$ (c) $M_{\mathrm{B}}=4 M_{\mathrm{A}}$ (d) $M_{\mathrm{B}}=2 M_{\mathrm{A}}$
Gaseous State
Exercises I
When $1 \mathrm{~g}$ of an ideal gas $\mathrm{A}$ is introduced into an evacuated vessel at $300 \mathrm{~K}$, the pressure was found to be 1 atm. Two grams of another ideal gas $\mathrm{B}$ is then added to $\mathrm{A}$ and the pressure is now found to be $1.5$ atm. What is the ratio between the average speeds of $A$ and $B$ at the same temperature? (a) $2: 1$ (b) $1: 2$ (c) $1: 4$ (d) $4: 1$
Exercises II
Pressure of 1 g of an ideal gas $A$ at $27^{\circ} \mathrm{C}$ is found to be 2 bar. When $2 \mathrm{~g}$ of another ideal gas $\mathrm{B}$ is introduced in the same flask at same temperature the pressure becomes 3 bar. Find a relationship between their molecular masses.
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