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Chapter 11 Gases

Chapter 11 Lecture. Basic Chemistry Fourth Edition. Chapter 11 Gases. 11.8 The Ideal Gas Law

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Chapter 11 Gases

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  1. Chapter 11 Lecture Basic Chemistry Fourth Edition Chapter 11 Gases 11.8 The Ideal Gas Law Learning Goal Use the ideal gas law equation to solve for P, V, T, or n of a gas when given three of the four variables in the ideal gas law equation. Calculate density, molar mass, or volume of a gas in a chemical reaction.

  2. The Ideal Gas Law PV = nRT The ideal gas law is a combination of the four properties (P, V, n, and T), written as a single expression: PV = nRT. Rearranging the ideal gas law equation shows that the four properties are equal to the gas law constant, R, equal to 0.0821 L atm per mol K.

  3. The Ideal Gas Law Using a different unit for pressure, 760 mmHg, gives us another value for R, 62.4 L mmHg, per mol K.

  4. Guide to Using the Ideal Gas Law

  5. Learning Check How many moles of N2 gas are present if the sample occupies 215 mL at 0.813 atm and 30.0 °C?

  6. Solution How many moles of N2 gas are present if the sample occupies 215 mL at 0.813 atm and 30.0 °C? Step 1State the given and needed quantities.

  7. Solution How many moles of N2 gas are present if the sample occupies 215 mL at 0.813 atm and 30.0 °C? Step 2Rearrange the ideal gas law equation to solve for the needed quantity.

  8. Solution How many moles of N2 gas are present if the sample occupies 215 mL at 0.813 atm and 30.0 °C? Step 3Substitute the gas data into the equation and calculate the needed quantity.

  9. Learning Check Butane, C4H10, is used as fuel for barbeques and as an aerosol propellant. If you have 108 mL of butane at 715 mmHg and 25 °C, what is the mass, in grams, of butane?

  10. Solution Given 108 mL of butane, C4H10, at 715 mmHg and 25 °C, what is the mass, in grams, of C4H10? Step 1State the given and needed quantities.

  11. Solution Given 108 mL of butane, C4H10, at 715 mmHg and 25 °C, what is the mass, in grams, of C4H10? Step 2 Rearrange the ideal gas law equation to solve for the needed quantity. Molar Mass moles of C4H10 grams of C4H10

  12. Solution Given 108 mL of butane, C4H10, at 715 mmHg and 25 °C, what is the mass, in grams, of C4H10? Step 3 Substitute the gas data into the equation and calculate the needed quantity.

  13. Molar Mass of a Gas Another use of the ideal gas law is to determine the molar mass of a gas. Dividing the mass of gas by the moles of gas gives the molar mass of the gas. Given the mass, in grams, of gas, we can calculate the number of moles of the gas using the ideal gas law equation.

  14. Guide to Calculating the Molar Mass of a Gas

  15. Learning Check What is the molar mass, in grams per mole, of a 3.16-g sample of gas at 0.750 atm and 45 °C, that occupies a volume of 2.05 liters?

  16. Solution What is the molar mass, in grams per mole, of a 3.16-g sample of gas at 0.750 atm and 45 °C, that occupies a volume of 2.05 liters? Step 1State the given and needed quantities.

  17. Solution What is the molar mass, in grams per mole, of a 3.16-g sample of gas at 0.750 atm and 45 °C, that occupies a volume of 2.05 liters? Step 2 Rearrange the ideal gas law equation to solve for the number of moles.

  18. Solution What is the molar mass, in grams per mole, of a 3.16-g sample of gas at 0.750 atm and 45 °C, that occupies a volume of 2.05 liters? Step 2 Rearrange the ideal gas law equation to solve for the number of moles.

  19. Solution What is the molar mass, in grams per mole, of a 3.16-g sample of gas at 0.750 atm and 45 °C, that occupies a volume of 2.05 liters? Step 3 Obtain the molar mass by dividing the given number of grams by the number of moles.

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