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Gases Chapters 12.1 and 13

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12.1 Main Idea Gases expand, diffuse, exert pressure, and can be compressed because they are in a low-density state consisting of tiny, constantly moving particles

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Objectives Predict the behavior of gases using the kinetic-molecular theory Explain how mass affects the rates of diffusion and effusion Calculate the partial pressure of a gas Measure gas pressure

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Review Vocabulary Kinetic energy Molar mass

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**New Vocabulary Kinetic-molecular theory Elastic collision Temperature**

Diffusion Graham’s Law Pressure Barometer Manometer Pascal (Pa) Dalton's law of partial pressure Atmosphere (atm)

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**Kinetic-Molecular (KM) Theory**

Assumptions Particle size is very small Particles take up relatively no space Particles are far apart Very little interaction of particles Collisions are elastic No kinetic energy is lost in a collision

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**Particle Energy Determined by mass and velocity**

Temperature- the average kinetic energy of particles in matter

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Behavior of Gases Pressure- gases will expand to fill the space they occupy

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Behavior of Gases Compression and expansion- density of material can be changed by changing the available volume

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**Behavior of Gases Diffusion- movement of one material through another**

Concentration gradient Effusion- gas escaping from a confined space through tiny openings

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**What is the ratio of the rate of diffusion for ammonia and hydrogen chloride?**

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**Calculate the ratio of effusion rates for nitrogen gas and neon**

RH/RHe = 0.849

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Pressure Pressure (P) is defined as the force per unit area on a surface. (P=F/A) Gas pressure is caused by collisions of the gas molecules with each other and with surfaces with which they come into contact. The pressure exerted by a gas depends on volume, temperature, and the number of molecules present. The greater the number of collisions of gas molecules, the higher the pressure will be.

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**Gas Pressure Barometer Manometer**

Barometers measure atmospheric pressure open system Manometers measure gas pressure in a closed system

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**Gas Pressure Units Pascal (1 Pa = 1 /m2)**

Atmosphere (1 atm = kPa) mm Hg (1 atm = 760 mm Hg) Torr (1 torr = 1 mm Hg)

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**Dalton’s Law of Partial Pressures**

total pressure is the sum of the partial pressures Ptot=P1 + P2 + P3 + … Pn

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**A mixture of O2, CO2 and N2 has a total pressure of 0. 97 atm**

A mixture of O2, CO2 and N2 has a total pressure of 0.97 atm. What is the partial pressure of O2 if the partial pressure of CO2 is 0.70 atm and the partial pressure of N2 is 0.12 atm? 0.97 atm = 0.70 atm atm + x X = 0.15 atm

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Can you… Predict the behavior of gases using the kinetic-molecular theory Explain how mass affects the rates of diffusion and effusion Calculate the partial pressure of a gas Measure gas pressure

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The Gas Laws Chapter 13.1

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13.1 Main Idea For a fixed amount of gas, a change in one variable- pressure, volume or temperature- affects the other two.

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13.1 Objectives State the relationships among pressure, volume, temperature, and the amount of gas Apply gas laws to problems involving pressure, volume, temperature, and the amount of gas Create graphs of the relationships among pressure, volume, temperature, and the amount of gas Solve problems related to fixed amounts of gases

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**Review Vocabulary Scientific law Directly related**

Indirectly (inversely) related Kelvin

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**New Vocabulary Ideal gas Absolute zero Boyle’s law Charles’s law**

Gay-Lussac’s law Combined gas law

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**Ideal gas Non-existent, but assumes the following:**

Completely elastic collisions Particles occupy no volume Large number of particles No attractive or repellent forces between particles Molecules are in completely random motion

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**Boyle’s Law Constants: amount of gas (n) and temperature (T)**

Boyle's Law in Motion

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**A diver blows a 0. 75 L air bubble 10 m under water**

A diver blows a 0.75 L air bubble 10 m under water. As it rises, the pressure goes from 2.25 atm to 1.03 atm. What is the volume of the bubble at the surface? P1V1=P2V2 2.25 atm 0.75 L = 1.6 L 1.03 atm

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**Charles’s Law Constants: amount of gas (n) and pressure (P)**

Temperature is in Kelvin (K) K= C Charles' Law in Motion

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**A helium balloon in a closed car occupies a volume or 2. 32 L at 40°C**

A helium balloon in a closed car occupies a volume or 2.32 L at 40°C. If the temperature rises to 75°C, what is the new volume of the balloon? V2=V1T2/T1 348.0 K 2.32 L = 2.58 L 313.0 K

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**Gay-Lussac’s Law Constants: amount of gas (n) and volume (V)**

T must be in Kelvin Gay-Lussac in Motion

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**The pressure of oxygen gas inside a canister is 5. 00 atm at 25°C**

The pressure of oxygen gas inside a canister is 5.00 atm at 25°C. the canister is placed in a cold environment where the temperature is -10°C; what is the new pressure in the canister? P2=P1T2/T1 263.0 K 5.00 atm = 4.41 atm 298.0 K

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Predict The relationship between pressure and amount of gas at a fixed temperature and volume Pressure-Moles relationship The relationship between volume and the amount of gas at a fixed temperature and amount of gas Volume-Moles relationship

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Combined Gas Law Combination of Boyle’s, Charles’, and Gay-Lussac’s laws

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A gas at 110 kPa and 30.0°C fills a flexible container with an initial volume of 2.00L. If the temperature is raised to 80.0°C and the pressure increases to 440 kPa, what is the new volume? 0.58 L

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**Gas Law Summary Law Boyle’s Charles’ Gay-Lussac’s Combined Formula**

Constant Moles, temp Moles, pressure Moles, volume Moles Graphic Volume Temperature Pressure Volume Temperature Pressure Volume Temperature Pressure Volume Temperature Pressure

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Can you… State the relationships among pressure, volume, temperature, and the amount of gas Apply gas laws to problems involving pressure, volume, temperature, and the amount of gas Create graphs of the relationships among pressure, volume, temperature, and the amount of gas Solve problems related to fixed amounts of gases

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Ideal Gas Law 13.2

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13.2 Main Idea The ideal gas law relates the number of particles to pressure, temperature, and volume

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13.2 Objectives Relate the number of particles and volume using Avogadro’s principle Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law Compare and contrast the properties of real gases and ideal gases Solve problems using the ideal gas law

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Review Vocabulary Mole Molar mass (M)

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**New Vocabulary STP Avogadro’s principle Molar volume**

Ideal gas constant (R) Ideal gas law

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**STP Standard temperature and pressure Standard temperature**

°C = K Standard pressure 1 atm = 760 torr = kPa

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Avogadro’s Principle Equal volumes of (ideal) gases, at the same temperature and pressure, contain equal numbers of particles 1 mol gas = 22.4 L at STP

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**How much volume do the following gases fill at STP**

1 mol CH4 1 mol CO2 1 mol H2O 1 mol Ne 2 mol He 1 mol O2

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Molar Volume The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00 kg of methane will occupy at STP. M = m/n M = molar mass m = mass n = number of moles

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The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00 kg of methane will occupy at STP. Molar mass (M) = g/mol (C + 4H)

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**Molar mass (M) = 16.05 g/mol (C + 4H) Number of moles (n) = ?? M = m/n **

The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00 kg of methane will occupy at STP. Molar mass (M) = g/mol (C + 4H) Number of moles (n) = ?? M = m/n n = m/M 2000 g CH4 1 mol = 125 mol 16.05 g

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**Molar mass (M) = 16.05 g/mol (C + 4H) Number of moles (n) = 125 mol**

The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00 kg of methane will occupy at STP. Molar mass (M) = g/mol (C + 4H) Number of moles (n) = 125 mol 2000 g CH4 1 mol = 125 mol 16.05 g

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**Molar mass (M) = 16.05 g/mol (C + 4H) Number of moles (n) = 125 mol **

The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00 kg of methane will occupy at STP. Molar mass (M) = g/mol (C + 4H) Number of moles (n) = 125 mol Molar volume = ?? 125 mol 22.4 L = 2800 L 1 mol

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**Ideal Gas Law PV=nRT P = pressure (atm) V = volume (L)**

n = number of moles of gas (mol) R = gas constant (L•atm)/(mol•K) T = temperature (K)

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**Calculate the number of moles of ammonia gas contained in a 3**

Calculate the number of moles of ammonia gas contained in a 3.0 L vessel at 300 K with a pressure of 1.50 atm. P = 1.50 atm; V = 3.0 L; n = ?; T = 300 K R = (L•atm)/(mol•K) N= PV/RT 1.50 atm (mol•K) 3.0 L = 0.18 mol (L•atm) 300 K

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Molar mass and density PV=nRT n=m/M PV=mRT/M M=mRT/PV D=m/V D=MV/RT

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**Ideal gas and Real gases**

Particles occupy no volume All collisions are perfectly elastic Infinitely large number of molecules No forces between molecules Particles occupy volume KE is lost during collisions Limited numbers of molecules Inter-molecular forces exist

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Can you… Relate the number of particles and volume using Avogadro’s principle Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law Compare and contrast the properties of real gases and ideal gases Solve problems using the ideal gas law

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Gas Stoichiometry 13.3

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Main Idea When gases react, the coefficients in the balanced chemical equation represent both molar amounts and the relative volumes.

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13.3 Objectives Determine volume ratios for gaseous reactants and products by using coefficients from chemical equations Apply gas laws to calculate amounts of gaseous reactants and products in a chemical reaction

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Review Vocabulary Stoichiometry Coefficient Chemical equation

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**Stoichiometry with Gases**

Only works with gases! 2H2 (g) + O2 (g) 2 H2O (g) 2 moles of hydrogen + 1 mole of oxygen react to form 2 moles of water 2 liters of hydrogen + 1 liter of oxygen react to form 2 liters of water

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**What volume of oxygen gas is needed for the complete combustion of 4**

What volume of oxygen gas is needed for the complete combustion of 4.00 L of propane gas assuming that pressure and temperature are constant? C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) 4.00 L C3H8 5 L O2 = 20.0 L O2 1 L C3H8

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Can you… Determine volume ratios for gaseous reactants and products by using coefficients from chemical equations Apply gas laws to calculate amounts of gaseous reactants and products in a chemical reaction

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Can you… Predict the behavior of gases using the kinetic-molecular theory Explain how mass affects the rates of diffusion and effusion Calculate the partial pressure of a gas Measure gas pressure State the relationships among pressure, volume, temperature, and the amount of gas Apply gas laws to problems involving pressure, volume, temperature, and the amount of gas Create graphs of the relationships among pressure, volume, temperature, and the amount of gas Solve problems related to fixed amounts of gases Relate the number of particles and volume using Avogadro’s principle Relate the amount of gas present to its pressure, temperature, and volume using the ideal gas law Compare and contrast the properties of real gases and ideal gases Solve problems using the ideal gas law Determine volume ratios for gaseous reactants and products by using coefficients from chemical equations Apply gas laws to calculate amounts of gaseous reactants and products in a chemical reaction

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GASES Chapter 12 in your text book. KINETIC-MOLECULAR THEORY OF GASES Gas particles are in constant random and rapid motion. The space between gas molecules.

GASES Chapter 12 in your text book. KINETIC-MOLECULAR THEORY OF GASES Gas particles are in constant random and rapid motion. The space between gas molecules.

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