A 2.00 g sample of gas fills up a 500 mL cylinder. The molar mass of the gas at SATP?
Volume of the gas=500mL=500×10−3L=0.5L=0.5dm3\textsf{Volume of the gas} = \\ 500mL = 500 \times 10^{-3} L = 0.5L = 0.5dm^3Volume of the gas=500mL=500×10−3L=0.5L=0.5dm3
Mass of the gas=2.00 g\textsf{Mass of the gas} = 2.00 \, gMass of the gas=2.00g
1 mole of gas=22.4dm31\textsf{ mole of gas} = 22.4dm^31 mole of gas=22.4dm3
xg=22.4dm32g=0.5dm3\begin{aligned} xg &= 22.4dm^3\\ 2g &= 0.5dm^3 \end{aligned}xg2g=22.4dm3=0.5dm3
x=2×22.40.5g=89.6gx = \dfrac{2 \times 22.4}{0.5}g = 89.6gx=0.52×22.4g=89.6g
∴\therefore∴ the molar mass of the gas at SATP is 89.6 g/mol89.6 \, g/mol89.6g/mol
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