Ideal Gas Law THEORY
Mention the general formula for the Ideal Gas Law
PV=nRT
P= 68 atm V= 581L n= 9.056 mol T= ?
T= (68 x 581) / (9.056 x 0.0821)
T= 53,138.03 K
If you have the following information, what variable would you be solving for?P1 = 720 torr, V1= 256mL, T1= 29°C, V2= 278mL and T2=43°C
Pressure 2 (P2)
If I initially have a gas at a pressure of 12 atm, a volume of 23 L and a temperature of 200K and then raise the pressure to 14 atm and increase the temperature to 300K, what is the new volume of the gas?
V2= (12 atm x 23L x 300K) / (14 atm x 200K)
V2= 29.6 L
Do we always use 0.0821 as the value of the variable R? (YES or NO)
Explain why.
Yes, because R is a constant and that means that it is always the same number. This number doesn't change unless different units are used.
A 22.9 mol sample of an unknown gas occupies a volume of 59 L at a pressure of 80 atm. What is the temperature? (Include units)
T= (80 x 59) / (22.9 x 0.0821)
T= 2,510.51 K
What formula would you use to calculate the original pressure?
P1= (P2 x V2 x T1) / (V1 x T2)
I have an unknown volume of gas at a pressure of 0.5 atom and a temperature of 325K. If I raise the pressure to 1.2 atm, decrease the temperature to 320K, and measure the final volume to be 48 L, what was the initial volume of the gas?
V1= (1.2 atm x 48L x 325K) / (0.5 x 320)
V1= 117 L
What happens when the temperature in the Ideal Gas Law is given in degrees Celsius (°C)?
We need to convert to Kelvin by adding 273
When we are calculating for Temperature, do we need to add 273 to our answer? YES or NO and why.
No, because when we calculate Temperature it is already in Kelvins.
Mention all the variables used in the ideal gas law.
P1, P2, T1, T2, V1, V2
If I have 2.9 L of gas a pressure of 5 atm and a temperature of 50°C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4L and decrease the pressure to 3 atm?
T2= (3 atm x 2.4 L x 323 K) / (5atm x 2.9L )
T2= 160.38 K
What does the variable R stand for in the Ideal Gas Law?
R= Gas Constant
What volume would 20 mol of CO2 occupy at 27 °C and 105 atm? (Make sure you include the units!!)
V= (20 x 0.0821 x 300) / 105
V= 4.69 L
Mention the units used in each one of the variables: Pressure, Volume and Temperature.
P= Atmospheres (atm) , V= Liters (L) and T= Kelvins (K)
Is I have 17L of gas at a temperature of 67°C and a pressure of 88.89 atm, what will be the pressure of the gas if I raise the temperature to 94°C and decrease the volume to 12L?
P2= (88.89 atm x 17L x 367.15K) / (12L x 340.15K)
P2= 136 atm
Describe what the ideal gas law states.
The Ideal Gas Law states that Pressure, Volume and Temperature of a gas are related.
What would be the number of moles for a substance that as 238 L at 634 atm and a -43 °C? (Include units)
n= (634 x 238) / (0.0821 x 230)
n= 7,990.89 mol
Which gas laws does the combined gas law include? (Mention all 3)
Gay Lussac, Boyle and Charles Gas Laws
A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K. If I raise the temperature to 350 K and lower the pressure to 1.5 atm, what is the new volume of the gas?
V2= (2.3 atm x 17L x 350K) / (1.5 atm x 259K)
V2= 30.5 L