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Gas Laws II.

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Presentation on theme: "Gas Laws II."— Presentation transcript:

1 Gas Laws II

2 STP Standard Temperature and Pressure 0⁰C 1atm

3 Dalton’s Law of Partial Pressures
The pressure of each gas in a mixture is called the partial pressure of that gas. Dalton’s law of partial pressures states that the total pressure of a gas mixture is the sum of the partial pressures of the component gases. Ptotal = P1 + P2 + P3 + ……

4 Gases produced in the laboratory are often collected over water
Water molecules at the liquid surface evaporate and mix with the gas molecules.

5

6 A container holds samples of O2, N2, and H2
A container holds samples of O2, N2, and H2. The pressure of the container is 2.1 atm. O2 exerts a pressure of 1.0atm and N2 exerts a pressure of 0.5atm, what is the pressure of the H2?

7 Oxygen gas from the decomposition of potassium chlorate, KClO3, was collected by water displacement. The barometric pressure and the temperature during the experiment were mmHg and 20.0°C. respectively. What was the partial pressure of the oxygen collected?

8 Ideal Gas Law the mathematical relationship among pressure, volume, temperature, and number of moles of a gas PV = nRT P= pressure V= volume in Liters n= number of moles R= ideal gas constant T= temperature in Kelvin

9 R Values

10 What is the pressure in atmospheres exerted by a 10
What is the pressure in atmospheres exerted by a g sample of nitrogen gas in a 10.0 L container at 298 K?

11 How many mol of CO2 gas are in a 2300mL container at 17⁰C and 2.14atm?

12 Gas Stoichiometry

13 Gas Stoichiometry The coefficients in chemical equations of gas reactions reflect not only molar ratios, but also volume ratios only if: ALL conditions remain the same Substances involved in calc are gases example—reaction of carbon dioxide formation: 2CO(g) O2(g)  2CO2(g) 2 molecules 1 molecule 2 molecules 2 mole 1 mole 2 mol 2 liters 1 liters 2 liters

14 C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g)
What will be the volume, in liters, of oxygen required for the complete combustion of L of propane? Assume that all volume measurements are made at the same temperature and pressure.

15 C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g)
What will be the volume of carbon dioxide produced by the complete combustion of L of propane? Assume that all volume measurements are made at the same temperature and pressure.

16 What if conditions are different or on substance is a solid or liquid?

17 For any gas at STP, 1mol = 22.41L If 5.60L H2 at STP reacts with excess CuO according to the equation below, how many g Cu are produced? CuO(s) + H2(g) → Cu(s) + H2O(g)

18 If 5.60L H2 at 3.16atm and 54 ⁰C reacts with excess CuO according to the equation below, how many g Cu are produced? CuO(s) + H2(g) → Cu(s) + H2O(g)

19 If 5.60L H2 at 1.21atm and 27 ⁰C reacts with excess CuO according to the equation below, what volume H2O(g) is produced at 1.74atm and 20.0⁰C? CuO(s) + H2(g) → Cu(s) + H2O(g)


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