Question
A sample of $\mathrm{O}_{2}(\mathrm{g})$ is collected over water at $24^{\circ} \mathrm{C}$.The volume of gas is 1.16 L. In a subsequent experiment, it is determined that the mass of $\mathrm{O}_{2}$ present is 1.46 g. What must have been the barometric pressure at the time the gas was collected? (The vapor pressure of water at $24^{\circ} \mathrm{C}$ is 22.4 Torr.)
Step 1
The molar mass of $\mathrm{O}_{2}$ is 32 g/mol. So, the number of moles of $\mathrm{O}_{2}$ is given by: \[n = \frac{m}{M} = \frac{1.46 \, \text{g}}{32 \, \text{g/mol}} = 0.0456 \, \text{mol}\] Show more…
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