Question

Topic: Practice exercise on gas laws. You must write the equation you are using to solve the exercise.

1. A sample of Argon gas occupies an initial volume of 5.40 L when its pressure is 6.52 atm. What will be the final pressure of the gas if its volume increases to 9.73 L?

2. An unknown gas occupies an initial volume of 0.256 L when its temperature equals 121ºC. What will be the final volume if the temperature drops to 25ºC?

3. A sample of a gas has an initial pressure equal to 744 mmHg when its initial temperature is 22ºC. What is the final temperature in degrees Celsius if the pressure increases to 766 mmHg?

4. A diver inhaled 50.0 mL of compressed air from his tank under the sea, which was at 3.00 atm pressure and 8ºC temperature. What is the final pressure in atmospheres (atm) if the gas in the lungs expands to 150.0 mL and the body temperature is 37ºC?

5. A container contains a mixture of the oxygen, nitrogen and helium gases. All these gases exert a total pressure in the container equal to 925 Torr. The partial pressure of oxygen is 425 Torr and that of helium is 75 Torr. What is the partial pressure of nitrogen in the mixture?

Answer 1

Andrer 1) According to boy According to Boyle's Law, we know if the temperature and the amount of a gas remains constant, then the pressure exerted by a gas will inversely proportional to the rolume. Mathematically, it can be expressed as, pat PV = constant So, it can be expressed as, Pivi - PzV2) --0 where, p = Initial pressure of the gas a Vi = Initial volume of the gas = 5.40L. P2 = Final pressure of the gas = ? V2 = Final volume of the gas = 9.73 L . Now putting the above values in equation 0 we get 6.52 atm x 5.404 = P2 x 9:734 ar, P = 6.52 x 5.40 ¿16 9.73 ..P2 = 3.618 atm. The final pressure of the gas = 3.618 atm. Cansurer) 97734