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.

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1. To find the final pressure of the air within the balloon, we can use the formula Boyle's Law. Boyle's Law states that for a fixed amount of gas at a constant temperature, the pressure and volume of the gas are inversely proportional. In equation form, it is expressed as P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

In this case, P1 = 0.120 atm, V1 = 2.31 L, and V2 = 7.14 L. We want to find P2.

Using the formula, we can rearrange it to solve for P2: P2 = (P1 * V1) / V2.

Substituting the given values: P2 = (0.120 atm * 2.31 L) / 7.14 L.

Calculating this expression gives us the final pressure P2. Round the answer to the nearest hundredth and add the appropriate units to obtain the final result.

2. To find the new pressure of the gas when the volume is increased, we can again use Boyle's Law. Using the same equation P1V1 = P2V2, where P1 = 2 atm, V1 = 8 L, and V2 = 10 L, we want to find P2.

Rearranging the formula, we have P2 = (P1 * V1) / V2.

Plug in the given values: P2 = (2 atm * 8 L) / 10 L.

Calculate the expression to find the pressure P2. Don't forget to include the appropriate units in the final answer.

3. To find the temperature in Kelvin when the gas expands to a new volume, we can use Charles's Law. Charles's Law states that for a fixed amount of gas at constant pressure, the volume and temperature of the gas are directly proportional. In equation form, it is expressed as V1 / T1 = V2 / T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

In this case, V1 = 10 L, V2 = 22 L, and T1 = 72 °C. We want to find T2 in Kelvin.

Using the formula, we can rearrange it to solve for T2: T2 = (V2 * T1) / V1.

Substituting the given values, T2 = (22 L * 72 °C) / 10 L.

Calculate this expression to find the temperature T2 in Kelvin. Round the answer to the nearest whole number and add the appropriate units.

4. Similar to question 3, we will use Charles's Law to find the temperature in Kelvin when the volume expands.

Given V1 = 14 L, V2 = 20 L, and T1 = 302 K, we want to find T2.

Using the formula, T2 = (V2 * T1) / V1.

Substituting the given values, T2 = (20 L * 302 K) / 14 L.

Calculate this expression to find the temperature T2 in Kelvin. Round the answer to the nearest whole number.

5. In this question, the volume is kept constant while the gas is cooled. We can use Gay-Lussac's Law, also known as the Pressure-Temperature Law, which states that if the volume of a gas is held constant, the pressure and temperature of the gas are directly proportional. In equation form, it is expressed as P1 / T1 = P2 / T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Given P1 = 750.0 mm Hg, T1 = 323.0 K, and T2 = 273.15 K, we want to find P2.

Rearranging the formula, we have P2 = (P1 * T2) / T1.

Plug in the given values: P2 = (750.0 mm Hg * 273.15 K) / 323.0 K.

Calculate the expression to find the pressure P2. Round the answer to the nearest tenth and add the appropriate units.

6. To find the final temperature of the gas in Kelvin after it is pressurized, we can use Gay-Lussac's Law again. Given P1 = 15.0 atm, P2 = 16.0 atm, and T1 = 25 °C, we want to find T2.

Using the formula, T2 = (P2 * T1) / P1.

Substituting the given values, we have T2 = (16.0 atm * 25 °C) / 15.0 atm.

Calculate this expression to find the temperature T2 in Kelvin. Round the answer to the nearest whole number and add the appropriate units.