A sample of gas has a mass of 0.565 g. Its volume is 117 mL at a temperature of 95 C and a pressure of 749 mm Hg. How would you find the molar mass of the gas?

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A sample of gas has a mass of 0.565 g. Its volume is 117 mL at a temperature of 95 C and a pressure of 749 mm Hg. How would you find the molar mass of the gas?

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Answer 1 · 2016-12-01T16:59:13

$Molar mass$ $"Molar mass"$ $≅$ $~=$ $150 \cdot g \cdot m o l^{- 1}$ $150*g*mol^-1$ .

Explanation:

From the Ideal Gas equation, $n = \frac{P V}{R T}$ $n=(PV)/(RT)$ , where, $n = \frac{Mass}{Molar mass}$ $n="Mass"/"Molar mass"$ .

And thus $Molar mass = \frac{Mass \times R T}{P V}$ $"Molar mass "=("Mass"xxRT)/(PV)$

$= \frac{0.565 \cdot g \times 0.0821 \cdot L \cdot a t m \cdot K^{- 1} \cdot m o l^{- 1} \times 368 \cdot K}{\frac{749 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}} \times 0.117 \cdot L} = ? ? ? g \cdot m o l^{- 1}$ $=(0.565*gxx0.0821*L*atm*K^-1*mol^-1xx368*K)/((749*mm*Hg)/(760*mm*Hg*atm^-1)xx0.117*L)=???g*mol^-1$

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A sample of gas has a mass of 0.565 g. Its volume is 117 mL at a temperature of 95 C and a pressure of 749 mm Hg. How would you find the molar mass of the gas?

1 Answer

Explanation:

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