Calculate the number of moles of oxygen gas collected by displacement of water at 14.0^{$\omicron $}C if the atmospheric pressure is 790 .Torr and the volume is 5.00 L.The vapor pressure of water at 14.0^{$\omicron $}C is 12.0 Torr. A) 0.0184 B) 4.46 C) 0.00335 D) 0.217 E) 0.224

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To find the number of moles of oxygen gas collected, we first need to calculate the partial pressure of the oxygen gas. The total atmospheric pressure is given as 790 Torr, and the vapor pressure of water at 14.0°C is 12.0 Torr. The partial pressure of oxygen is the difference between these two pressures: 790 Torr - 12 Torr = 778 Torr.Next, we convert the pressure to atmospheres since the ideal gas law uses pressure in atmospheres: 778 Torr * (1 atm / 760 Torr) = 1.024 atm.We can now use the ideal gas law, PV = nRT, to solve for the number of moles (n) of oxygen gas. Rearranging the equation gives us n = PV / RT. The volume (V) is given as 5.00 L, R (the ideal gas constant) is 0.0821 L·atm/(mol·K), and the temperature (T) must be converted to Kelvin: 14.0°C + 273.15 = 287.15 K.Plugging in the values gives us n = (1.024 atm * 5.00 L) / (0.0821 L·atm/(mol·K) * 287.15 K) = 0.217 moles.

Calculate the Number of Moles of Oxygen Gas Collected by Displacement