1.If the pressure of the gas in a 2.31 L balloon is 0.120 atm and the volume increases to 7.14 L, what will be the final pressure of the air within the balloon? Round to the nearest hundredth. Don't forget the units.

2.At a pressure of 2 atm, hydrogen gas occupies a volume of 8 L. What pressure must the gas be under if the volume is increased to 10 L? Don't forget the units.

3.A gas at 72 °C occupies 10 L. What is the temperature in Kelvin when it expands to a volume of 22 L? Round to the nearest whole number and don't forget the units.

4.A balloon is filled with 14 L of gas at 302 K. What is its temperature in Kelvin when the volume expands to 20 L? Round to the nearest whole number. Don't forget the units.

5.If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant, what final pressure would result if the original pressure was 750.0 mm Hg? Round to the nearest tenth. Don't forget the units.

6.If a gas in a closed container is pressurized from 15.0 atm to 16.0 atm and its original temperature was 25 °C, what would be the final temperature of the gas in Kelvin? Round to the nearest whole number. Don't forget the units.

All of these can be worked with

(P1V1/T1) = (P2V2/T2)

1. To find the final pressure of the air within the balloon, you can use the combined gas law equation:

P1V1/T1 = P2V2/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.

In this case, we have:
P1 = 0.120 atm
V1 = 2.31 L
V2 = 7.14 L

We need the initial and final temperatures to solve the equation. However, since the temperature is not given, we cannot determine the final pressure without further information.

2. To find the pressure the gas must be under when the volume is increased to 10 L, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

In this case, we have:
P1 = 2 atm
V1 = 8 L
V2 = 10 L

We need the initial and final temperatures to solve the equation. However, since the temperature is not given, we cannot determine the final pressure without further information.

3. To find the temperature in Kelvin when the gas expands to a volume of 22 L, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

In this case, we have:
V1 = 10 L
V2 = 22 L

We need the initial and final pressures to solve the equation. However, the pressure is not given, so we cannot determine the temperature without further information.

4. To find the temperature in Kelvin when the volume expands to 20 L, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

In this case, we have:
V1 = 14 L
V2 = 20 L

We need the initial and final pressures to solve the equation. However, the pressure is not given, so we cannot determine the temperature without further information.

5. To find the final pressure when the gas is cooled from 323.0 K to 273.15 K and the volume is kept constant, we can use the ideal gas law equation:

P1V1/T1 = P2V2/T2

In this case, we have:
P1 = 750.0 mm Hg
T1 = 323.0 K
T2 = 273.15 K

We need the initial volume and final pressure to solve the equation. However, the volume is not given, so we cannot determine the final pressure without further information.

6. To find the final temperature of the gas in Kelvin when it is pressurized from 15.0 atm to 16.0 atm and the initial temperature is 25 °C, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

In this case, we have:
P1 = 15.0 atm
P2 = 16.0 atm
T1 = 25 °C

To convert °C to Kelvin, we can use the equation:
T(K) = T(°C) + 273.15

T2 = T1 * (P2/P1)

Substituting the given values:
T2 = (25 + 273.15) * (16.0/15.0)

Calculate the final temperature to the nearest whole number using the formula above.