A mixture of 12.7 g of O2 and 51.7 g of Ar is placed in a 100.0 L container at 330 K. What is the partial pressure of O2 in atmospheres? Express your answer with the appropriate units.

To find the partial pressure of O2 in a mixture, calculate the moles of O2 and the total pressure of the mixture using the ideal gas law equation. Divide the mass of O2 by its molar mass to get the moles of O2, and use the ideal gas law equation P = nRT/V to find the total pressure. Plug in the values to calculate the partial pressure of O2. Therefore, the partial pressure of O2 in the mixture is 0.1084545 atm.

Explanation:

To find the partial pressure of O2, we need to calculate the moles of O2 and the total pressure of the mixture. First, let's calculate the moles of O2. To do this, we divide the mass of O2 by its molar mass, which is 32 g/mol. 12.7 g of O2 divided by 32 g/mol gives us 0.3975 mol of O2. Now, let's calculate the total pressure of the mixture using the ideal gas law. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Rearranging the equation to solve for P, we get P = nRT/V. Plugging in the values, we have P = (0.3975 mol)(0.0821 L·atm/(mol·K))(330 K)/(100.0 L) = 0.1084545 atm. Therefore, the partial pressure of O2 in the mixture is 0.1084545 atm.

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