Boyle’s Law
Which of the following variables are held constant in Boyle’s Law?
Temperature and Number of Moles
What two variables are involved in Charles’s Law?
Volume and Temperature
Which two variables are involved in Gay-Lussac’s Law?
Pressure and Temperature
What unit must temperature be in?
Kelvin(k)
What does “R” stand for in the Ideal Gas Law?
Ideal gas constant
According to Boyle’s Law, what happens to volume when pressure increases (at constant temperature)?
Volume decreases
Charles’s Law requires temperature to be in what unit?
Kelvin(k)
What happens to pressure if temperature increases?
Pressure increases
What is the formula for the Combined Gas Law?
(P₁V₁)/T₁ = (P₂V₂)/T₂
What is the Ideal Gas Law formula?
PV = nRT
What must remain constant in order to apply Boyle’s Law?
Temperature
What happens to volume when temperature increases, according to Charles’s Law?
Volume increases
What stays constant in Gay-Lussac’s Law?
Volume
What condition must stay constant in the Combined Gas Law?
Number of moles(Gas)
What units are used for volume in the Ideal Gas Law
Liters(L)
Boyle’s Law is an example of what kind of relationship: direct or inverse?
Inverse
Charles’s Law assumes which variable stays constant?
Pressure
what is the formula for Gay-Lussac’s Law
P₁/T₁ = P₂/T₂
In the Combined Gas Law, if the temperature increases and pressure stays the same, what must happen to the volume?
Volume increases
In the Ideal Gas Law, this variable represents the number of moles of gas and is used to calculate how much substance is present in a sample.
n
At a constant temperature, 4.0 liters of hydrogen gas are compressed to 0.30 liters. The new pressure of the gas is 7.0 atm. 7.0 atm is your P2! Determine the pressure of the gas before it was compressed. *Round to the nearest hundredths place! i.e. 50.36
0.53 atm( p1= 7.0⋅0.30/4.0=2.1/4.0=0.525 rounds to 0.53atm)
The gas inside a hot air balloon occupies 4.10 L at 310 K. At what temperature will the balloon expand to 6.15 L? Round your answer to the nearest whole number!
466 K
t2=(6.15)(310)/(4.10)=(1906.5)(4.10)=465.98
A sample of gas has a pressure of 4.5 atm and a temperature of 52 °C. What will be the new pressure if the temperature is raised to 227 °C? *Round to the nearest hundredths place! i.e. 50.62
6.92atm
A gas has 2.0 L at 1.0 atm and 300 K. What is the volume at 2.0 atm and 400 K?
1.5 L (P₁V₁/T₁ = P₂V₂/T₂ → (1×2)/300 = (2×V₂)/400 → V₂ = 1.5 L)
At what temperature (in Kelvin) would 3.00 moles of oxygen gas exert a pressure of 1.85 atm in a 30.0 L container? (Round your answer to the hundredths place.)
225.42 K
T=(1.85)(30.0)/(3.00)(0.0821)=55.5/0.2463=225.42K