1.Suppose you have a container filled with air at 212 oF. The volume of the container 1.00 L, the pressure of air is 1.00 atm. The molecular composition of air is 79% N2 and 21% O2 for simplification. Calculate the mass of air and moles of O2 in the container.moles of O2=.006 and moles of N2=.025 moles   2.A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container(total mass of air=.892) , according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container? I need help with finding the new total pressure for question 2.

Question

1.Suppose you have a container filled with air at 212 oF. The volume of the container 1.00 L, the pressure of air is 1.00 atm. The molecular composition of air is 79% N2 and 21% O2 for simplification. Calculate the mass of air and moles of O2 in the container.moles of O2=.006 and moles of N2=.025 moles

2.A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container(total mass of air=.892) , according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container?

I need help with finding the new total pressure for question 2.