10. Gas Formulas = = Pressure)(Volume) = (moles)(Ideal Gas Constant)(Temperature) PV = nRT Total pressure of a gas = sum of the partial pressures of the component gas P t = P 1 + P 2 + P 3 +…
11.
12. Two flasks are connected by a stopcock as shown below. The 5.0 L flask contains CH 4 at a pressure of 3.0 atm, and the 1.0 L flask contains C 2 H 6 at a pressure of 0.55 atm. Calculate the pressure of CH 4 after the stopcock is opened. Assume that the temperature remains constant.
13. Gas Law Problems What conversions are necessary? Variable Quantity Conversions P V n T
14. What would be the mass of 400. mL of hydrogen collected at 20 ° C and 740 torr?
15. P t = P 1 + P 2 + P 3 +… A gaseous mixture containing 1.5 moles argon and 3.5 moles of carbon dioxide has a total pressure of 7.0 atm. What is the partial pressure of carbon dioxide?