An $0.846 \cdot g$ $0.846g$ mass of gas exerts a pressure of $752 \cdot Torr$ $752"Torr"$ , and expresses a volume of $354 \cdot m L$ $354*mL$ , at a temperature of $100$ $100$ $^{\circ} C$ $""^@C$ . What is the molar mass of the gas?

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An $0.846 \cdot g$ $0.846g$ mass of gas exerts a pressure of $752 \cdot Torr$ $752"Torr"$ , and expresses a volume of $354 \cdot m L$ $354*mL$ , at a temperature of $100$ $100$ $^{\circ} C$ $""^@C$ . What is the molar mass of the gas?

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Answer 1 · 2017-04-20T06:18:18

$\frac{Mass}{Molar mass} = \frac{P \times V}{R \times T}$ $"Mass"/"Molar mass"=(PxxV)/(RxxT)$ ; from where did I get this relationship?

Explanation:

And thus $Molar mass = \frac{R \times T \times mass}{P \times V}$ $"Molar mass"=(RxxTxx"mass")/(PxxV)$

$= \frac{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 373 \cdot K \times 0.846 \cdot g}{\frac{752 \cdot Torr}{760 \cdot Torr \cdot a t m^{- 1}} \times 0.354 \cdot L}$ $=(0.0821*(L*atm)/(K*mol)xx373*Kxx0.846*g)/((752*"Torr")/(760*"Torr"*atm^-1)xx0.354*L)$

$≅ 74 \cdot g \cdot m o l^{- 1}$ $~=74*g*mol^-1$

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An $0.846 \cdot g$ $0.846g$ mass of gas exerts a pressure of $752 \cdot Torr$ $752"Torr"$ , and expresses a volume of $354 \cdot m L$ $354*mL$ , at a temperature of $100$ $100$ $^{\circ} C$ $""^@C$ . What is the molar mass of the gas?

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An 0.846⋅g0.846*g mass of gas exerts a pressure of 752⋅Torr752*"Torr", and expresses a volume of 354⋅mL354*mL, at a temperature of 100100 ∘C""^@C. What is the molar mass of the gas?

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An $0.846 \cdot g$ $0.846g$ mass of gas exerts a pressure of $752 \cdot Torr$ $752"Torr"$ , and expresses a volume of $354 \cdot m L$ $354*mL$ , at a temperature of $100$ $100$ $^{\circ} C$ $""^@C$ . What is the molar mass of the gas?