Physical Science Gas Laws Test

Boyles Law: P1/V1 = P2/V2 1atm = Standard Pressure

Charles Law: V1/T1 = V2/T2 Degrees Celcius + 273 = Kelvin

Combined gas Law: (P1) (V1) = (P2) (V2)

(T1) (T2)

Answer the following problems using the correct formula. Show your work and include the correct unit of measure. You must Identify the law you are using for each problem.

1. A gas occupies 4.31 litres at a pressure of 0.755atm. Determine the volume if the pressure is increased to 1.25 atm.

2. 600 mL of a gas is at a pressure of 8.00atm. What is the Volume of the gas at 2 atm?

3. How hot will a 2.3 L balloon have to get to expand to a volume of 400 L? Assume that the initial temperature of the balloon is 25 degrees Celsius.

4. A gas takes up a volume of 17 litres, has a pressure of 2.3atm, and a temperature of 299K. If I raise the temperature to 350K and lower the pressure to 1.5atm, what is the new volume of the gas?

Question

Francisco Cantu

Chemistry

1 November, 00:00

Physical Science Gas Laws Test

Boyles Law: P1/V1 = P2/V2 1atm = Standard Pressure

Charles Law: V1/T1 = V2/T2 Degrees Celcius + 273 = Kelvin

Combined gas Law: (P1) (V1) = (P2) (V2)

(T1) (T2)

Answer the following problems using the correct formula. Show your work and include the correct unit of measure. You must Identify the law you are using for each problem.

1. A gas occupies 4.31 litres at a pressure of 0.755atm. Determine the volume if the pressure is increased to 1.25 atm.

2. 600 mL of a gas is at a pressure of 8.00atm. What is the Volume of the gas at 2 atm?

3. How hot will a 2.3 L balloon have to get to expand to a volume of 400 L? Assume that the initial temperature of the balloon is 25 degrees Celsius.

4. A gas takes up a volume of 17 litres, has a pressure of 2.3atm, and a temperature of 299K. If I raise the temperature to 350K and lower the pressure to 1.5atm, what is the new volume of the gas?

+2

Answers (1)

Know the Answer?

Sammy Dean · Answer 1

1. A gas occupies 4.31 litres at a pressure of 0.755atm. Determine the volume if the pressure is increased to 1.25 atm.

method: Boyles Law : P1/V1 = P2/V2

P1/V1 = P2/V2 implies V2 = P2 V1 / P1

V2=1.25x4.31 / 17=7.13L

2. 600 mL of a gas is at a pressure of 8.00atm. What is the Volume of the gas at 2 atm?

method: Boyles Law: P1/V1 = P2/V2

P1/V1 = P2/V2 implies V2 = P2 V1 / P1,

V1=2.6mL=0.026L

V2 = P2 V1 / P1 = 0.00065 L

3. How hot will a 2.3 L balloon have to get to expand to a volume of 400 L? Assume that the initial temperature of the balloon is 25 degrees Celsius.

Method: Charles Law: V1/T1 = V2/T2 Degrees Celcius + 273 = Kelvin

25 degrees Celsius=25+273=298K=T1

V1=2.3L, V2=400L

V1/T1 = V2/T2 implies T2=V2T1/V1 = (400x298) / 2.3=51826 K

4. A gas takes up a volume of 17 litres, has a pressure of 2.3atm, and a temperature of 299K. If I raise the temperature to 350K and lower the pressure to 1.5atm, what is the new volume of the gas?

Combined gas Law: (P1) (V1) = (P2) (V2)

(T1) (T2)

V1=17L

P1=2.3 atm

T1 = 299K

P2=1.5 atm

T2=350 K

V2=?

(P1) (V1) / T1 = (P2) (V2) / T2

so V2 = (P1) (V1) T2 / P2 T1

V2=17x2.3x350 / 1.5 x 299 = 30.51L