A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 degrees C and a pressure of 753 mmHg. What is the molar mass of the gas?

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A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 degrees C and a pressure of 753 mmHg. What is the molar mass of the gas?

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Answer 1 · 2017-11-18T08:02:16

We solve the Ideal Gas equation......and we know that $1 \cdot a t m$ $1*atm$ will support a column of mercury that is $760 \cdot m m$ $760*mm$ high.....

i.e. $1 \cdot a t m \equiv 760 \cdot m m \cdot H g$ $1*atm-=760*mm*Hg$

Explanation:

$n = \frac{P V}{R T} = \frac{Mass}{Molar mass}$ $n=(PV)/(RT)="Mass"/"Molar mass"$

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

$\frac{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 358.1 \cdot K \times 0.555 \cdot g}{\frac{753 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}} \times 0.117 \cdot L} = ? ? \cdot g \cdot m o l^{- 1}$ $(0.0821*(L*atm)/(K*mol)xx358.1*Kxx0.555*g)/((753*mm*Hg)/(760*mm*Hg*atm^-1)xx0.117*L)=??*g*mol^-1$ ....

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A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 degrees C and a pressure of 753 mmHg. What is the molar mass of the gas?

1 Answer

Explanation:

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