Gas Stoichiometry
What are the conditions at Standard Temperature and Pressure?
Temperature = 273 K or 0oC
Pressure = 1 atm
Which gas law supports the following scenario:
A balloon with given amount of gas has a set volume, at constant temperature and pressure. The balloon springs a leak and the volume decreases.
Which gas law describes this situation?
Avogadro's Law relates volume and moles of substance to one another.
(V1)/(n1) = (V2)/(n2)
What is the name and the equation you would use to find the partial pressure of a gas given the total pressure of the gas mixture and the other partial pressures of the gases in the mixture?
Dalton's Law
PTotal = P1 + P2 + P3 +...
According to Boyle's law, if the volume of a gas is halved while its temperature is kept constant, what happens to the pressure?
The pressure would double.
Boyle's Law
P1V1 = P2V2
A sample of gas has a volume of 2.0 L, a pressure of 1.0 atm, and a temperature of 300 K. If the volume is increased to 4.0 L and the temperature is decreased to 200 K, what is the new pressure according to the ideal gas law?
(P1V1)/(T1) = (P2V2)/(T2)
(P2) = (P1V1T2)/(T1V2)
(P2) = (1.0atmx2.0Lx200K)/(300Kx4.0L)
(P2) = 0.33 atm
Determine the volume in Liters of 0.85 moles of Oxygen gas at STP.
19.04 Liters O2
Which gas law supports the following scenario:
A scuba diving oxygen tank has a constant amount of oxygen at a constant temperature. As a diver takes the tank deeper below the surface and the pressure increases, the volume of gas decreases.
Which gas law describes this situation?
Boyle's Law relates pressure and volume.
P1 V1 = P2 V2
What is the name and the equation you would use to find the initial pressure of a gas given the initial temperature, the final temperature, and the final pressure?
Gay-Lussac's Law
(P1)/(T1) = (P2)/(T2)
According to Charles' Law, if the temperature of a gas is doubled while its pressure is kept constant, what happens to the volume?
The Volume doubles as well.
Charles' Law
(V1)/(T1) = (V2)/(T2)
What is the volume of 0.5 moles of a gas at a pressure of 7.0 atm and 290 K.
PV = nRT
V = (nRT)/(P)
V = (0.5molx0.0821(Latm/molK)x290K)/(7.0atm)
V = 1.70 L
Determine the mass in grams of 50.0 L of CO2 gas at STP.
98.24 grams CO2
Given the following scenario, determine how the change in one gas factor will change the other.
A pressure cooker works because of Gay-Lussac's Law. As a pressure cooker increases the internal pressure, what is happening to the internal temperature? Assume constant volume and amount of gas.
The temperature increases as well.
Gay-Lussac's Las says that pressure and temperature is directly related.
State the equation for Charles' Law and what two factors must be held constant in order to use Charles' Law.
Charles's Law
(V1)/(T1) = (V2)/(T2)
Constants:
1. Pressure
2. Amount of Substance
A sample of gas has a volume of 2.0 L and a pressure of 1.0 atm. If the volume is decreased to 1.0 L while the temperature is kept constant, what is the new pressure of the gas?
(P1V1) = (P2V2)
(P2) = (P1V1)/(V2)
(P2) = (1.0atm x 2.0L)/(1.0L)
(P2) = 2.0 atm
What are the units of pressure, volume, and temperature in the ideal gas law equation?
Due to the R constant, the following units are:
Temperature : Kelvins (K)
Pressure : Atmospheres (atm)
Volume : Liters (L)
R = 0.0821 (L atm)/(mol K)
Using the reaction below, determine the volume of Chlorine gas produced if 1.75 moles of KCl go into the reaction.
4 KCl + O2 --> 2 K2O + 2 Cl2
19.6 Liters of Chlorine gas
Given the following scenario, determine how the change in one gas factor will change the other.
A carbonated bottle of soda in a garage freezes. What happens to the volume of gas inside the bottle of soda? Assume constant pressure and amount of substance.
Determine what the change in volume will be as well as the Gas Law that justifies this change.
Charles' Law states that volume and temperature are directly related. The volume will decrease the in the soda bottle.
What is the name and the equation you would use to find the moles of a gas given the pressure, temperature, and volume of the gas?
Ideal Gas Law
PV=nRT
A sample of gas has a final pressure of 2.5 atm and a temperature of 300 K. If the initial temperature was 400 K and the volume is kept constant, what is the initial pressure of the gas?
(P1)/(T1) = (P2)/(T2)
(P1) = (P2T1)/(T2)
(P2) = (2.5 atm x 400K)/(300K)
(P2) = 3.33 atm
A gas has a pressure of 2.0 atm and a volume of 5.0 L at 27°C. What is the new volume of the gas if the pressure is decreased to 1.5 atm and the temperature is increased to 37°C?
(P1V1)/(T1) = (P2V2)/(T2)
(V2) = (P1V1T2)/(T1P2)
(V2) = (2.0atmx5.0Lx300K)/(310Kx1.5atm)
(V2) = 6.45 L
If 27.0 L of Oxygen gas go into the reaction, how many grams of K2O will be produced?
4 KCl + O2 --> 2 K2O + 2 Cl2
227.09 g K2O
Given the following scenario, determine how the change in one gas factor will change the other.
As you climb a mountain and increase your elevation, atmospheric pressure drops. Describe what happens to the temperature of the air as your elevation increases.
Determine what the change in temperature will be as well as the Gas Law that justifies this change.
Gay-Lussac's Law states that Pressure and Temperature are directly proportional, so as Pressure decrease, the temperature of the air decreases as well.
What is the name and the equation you would use to find the initial volume of a gas given the initial temperature, initial pressure, final temperature, final volume, and final pressure?
State what factor must be held constant in order to use this equation.
Combined Gas Law
Equation:
Constant: Moles/Amount of Substance
A sample of gas has a volume of 2.2 L and a temperature of 30 oC. If the volume is increased to 4.7 L while the pressure is kept constant, what is the new temperature (in Celsius) of the gas?
(V1)/(T1) = (V2)/(T2)
(T2) = (V2T1)/(V1)
(T2) = (4.7L x 303K)/(2.2L)
(T2) = 647.32 K - 273
(T2) = 374.32 C
A sample of gas has a volume of 2.52 L at a pressure of 1.91 atm and a temperature of 27°C. What is the number of moles of gas in the sample?
PV = nRT
n = (PV)/(RT)
n = (1.91atmx2.52L)/(0.0821(Latm/molK)x300K)
n = 0.195 mol