A gas mixture contains 74% nitrogen and 26% oxygen. If the total pressure is 1.05 atm what are the partial pressures of each component? Express your answers using two significant figures.

According to Dalton's law of partial pressures, that states the total pressure of a mixture of gases is the sum of the partial pressures of individual gases in the mixture, and the ideal gas law that states at constant temperature and volume, the partial pressure of gases in a mixture is the same as the proportion of the number of moles of them, we can solve this problem.

If the molar percents of the nitrogen and oxygen in the mixture are 74, and 26%, respectively, thus we can assume that the partial pressures of them are also at the same proportion. Combining this with Dalton's law would give:

Pnitrogen=0.74×1.05=0.78atmPnitrogen=0.74×1.05=0.78atm

and

Poxygen=0.26×1.05=0.27atmPoxygen=0.26×1.05=0.27atm

where's the diagram?