 If I have an unknown quantity of N 2 held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams of N 2 do I have?

Unit 8, Day 7 Kimrey 4 December 2012

 When you use Kelvin, you will never have a negative temperature!  Absolute zero (the coldest temperature possible) occurs at 0 K

 1 mole = 22.4 L of a gas at STP  STP = 0°C and 1 atm

 How many liters of Nitrogen gas are there in 4.56 moles?  How many liters of fluorine are there in 56.7 grams?

N 2 + H 2  NH 3  64.0 L of nitrogen will produce how many liters of ammonia (at STP)?  Don’t forget to balance!!!

2H 2 + O 2  2H 2 O  How many liters of water will be produced from 15 moles of oxygen?

2H 2 + O 2  2H 2 O  How many liters of water will be produced from 100 grams of Hydrogen gas if Oxygen gas is in excess?

2H 2 + O 2  2H 2 O  How many liters of water will be produced from 300 grams of Oxygen gas if Hydrogen gas is in excess?

Unit 8, Day 8 Kimrey 4 December 2012

 When you use Kelvin, you will never have a negative temperature!  Absolute zero (the coldest temperature possible) occurs at 0 K

 In a mixture of gases, each gas has a partial pressure ◦ The pressure that the gas would have if it alone occupied the same volume and temperature as the mixture

 The total pressure of a mixture is equal to the sum of all the partial pressures of each gas.  P total = P 1 + P 2 + P 3 + …

 What is the total pressure of a mixture of oxygen and hydrogen, if the partial pressure of oxygen is 4.5 atm and the partial pressure of hydrogen is 6.7 atm?  Total pressure = 11.2 atm

 What is the partial pressure of nitrogen in a mixture of nitrogen, hydrogen, and oxygen if the total pressure is found to be atm and the partial pressure of oxygen is 7.5 atm and the partial pressure of hydrogen is 6.7 atm?  N 2 Pressure = – ( ) = 6.56 atm

 What is the total pressure of a mixture of CO 2 and O 2, if the partial pressure of oxygen is kPa and the partial pressure of hydrogen is 6.7 atm?

 What is the partial pressure of nitrogen in a mixture of nitrogen, hydrogen, and oxygen if the total pressure is found to be atm and the partial pressure of oxygen is 17.5 atm and the partial pressure of hydrogen is 7.45 atm?  If I have a container that contains both oxygen and nitrogen, what’s the total pressure inside the container of the partial pressure of oxygen is 0.50 atm and the partial pressure of nitrogen is 0.75 atm?

 Given moles of specific gases, you can solve for individual pressures then add them up for the total pressure

 15 moles of nitrogen gas, 12 moles of oxygen gas, and 22 moles of hydrogen gas are mixed in a 25 liter flask at a temperature of 300 K. What are the partial pressures of each gas and the total pressure of the mixture? 1. Use the ideal gas law to find each gas’ partial pressure 2. Add up the pressures for the total pressure

 Given moles of specific gases, you can solve for individual pressures then add them up for the total pressure  Using the combined gas law, you can determine the pressure of a mixture given initial conditions

The stopper between a 3.00 L bulb containing oxygen at 295 torr and a 1.00 L bulb containing nitrogen at 530 torr is opened. What is the total pressure of the mixture (assume constant T = 298 K)?  P tot = P oxygen + P nitrogen  You can treat each gas separately.  After mixing, there will be the same number of moles of each gas, at the same T, just in a different volume.

 A mixture of hydrocarbons contains seven moles of methane, four moles of ethane, and three moles of propane. The container has a volume of 124 liters and the temperature is 22 °C. Find the partial pressures of the three gases, in atm.

 Given moles of specific gases, you can solve for individual pressures then add them up for the total pressure  Using the combined gas law, you can determine the pressure of a mixture given initial conditions  By comparing moles of each gas, as well as having a total pressure, you can calculate partial pressures

 What is the partial pressure of each gas in a mixture which contains 40 g of He, 56 g of N 2, and 16 g of O 2, if the total pressure of the mixture is 5 atmospheres? 1. Convert each gas to moles 2. Determine the fraction of moles of each gas (mole of gas / total moles) 3. Multiply the fractions by the total pressure