Styrene oxide is a fairly simple aromatic organic compound that has a pleasant odor and is often used in the perfume industry. If 2.07 g of the compound is vaporized completely into a closed 1.04 L flask at 435 oC, the pressure in the flask is found to be 735 torr. Calculate the formula weight of styrene oxide.

The mass percent of a three component gas sample is 6.40% C2H4, 38.2% C4H8 and 55.4% N2H4. Calculate the partial pressure (torr) of C2H4 if the total pressure of the sample is 258.4 torr.

A sample of gas of mass 3.22 g  occupies a volume of 442 mL  at 58 oC  and 0.18 atm  pressure. What is the molar mass of the gas?

Please don't provide handwritten solution....

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.05 atm, and the mole fraction of O2 in air is 0.210.

If 1.27 g Ar are added to 1.17 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of the resulting gaseous mixture?

The mass percent of a three component gas sample is 40.8% B4H8, 14.4% C2H4O2 and 44.8% C2H4F2. Calculate the partial pressure (torr) of C2H4O2 if the total pressure of the sample is 0.620 atm.