Warm Up #3 You are given a 5000.0 mL container of SO2 gas with a pressure of 1.4 atm. If the temperature of this gas is at 25oC, how much gas will you.

Slides:

Advertisements

Similar presentations

Unit 4 Sections A14a-c In which you will learn about: Combined gas law Dalton’s law Graham’s Law.

Advertisements

Three More Laws. A. Ideal Gas Law The 4 th variable that considers the amount of gas in the system is P 1 V 1 T 1 n = P 2 V 2 T 2 n Equal volumes of gases.

Gases: Mixtures and Movements

Gas Volumes and Ideal Gas Law. Up to this point, the gas laws have kept the amount of gas (moles) the same.

Molecular Composition of Gases

NOTES: 14.4 – Dalton’s Law & Graham’s Law

Gas Laws REVIEW GAME. Question 1 A 4.3 liter tank of hydrogen is at a pressure of 6.2 atmospheres. What volume of hydrogen will be available if the hydrogen.

Chapter 11 Gases.

 The average kinetic energy (energy of motion ) is directly proportional to absolute temperature (Kelvin temperature) of a gas  Example  Average energy.

Chapter 12 (Practice Test)

Chapter 14: The Behavior of Gases

Chapter Gases: Mixtures and Movements. The surface of a latex balloon has tiny pores through which gas particles can pass. The rate at which.

Starter S-146 List five properties of gases.. The Behavior of Gases Chapter 14.

Ideal Gas Law & Gas Mixtures. Ideal Gas Law Ideal Gas Law: PV = nRT Where n = the number of moles R is the Ideal Gas Constant The ideal gas law can be.

Do Now & Announcements Turn in Lab from yesterday Take out notes from yesterday—you can staple it to today’s packet as these are the notes for the entire.

Remember according to Avogadro’s law, one mole of any gas will occupy the same volume as one mole of any other gas at the same temperature regardless.

Pressure, temperature and volume relationships (w/ a constant amount of molecules As pressure, the volume_____ –Therefore, the relationship is ______________.

Chapter 14 Gas Laws Kinetic Molecular Theory – Assumes gas particles are small particles w/lots of space between them – No attractive forces; particles.

For your lab… What should you have in your conclusion? What is the point of “concluding”?

Ch. 14 The Behavior of Gases PROPERTIES OF GASES.

1. Identify the four factors that affect gases. Pressure Volume Number of moles Temperature a. b. c. d. P V n T (Kelvin)

Dalton’s Law P t = P 1 +P 2 +P 3 + ….. constant V & T)

Jennie L. Borders. Section 14.1 – Properties of Gases Compressibility is a measure of how much the volume of matter decreases under pressure. Gases are.

DALTON’S LAW GRAHAM’S LAW GAS MIXTURES. THINK ABOUT THIS Two students in the classroom bring a bottle of cologne and a bottle of perfume to the classroom.

Dalton’s Law of Partial Pressures P total =P 1 +P 2 +…. Total pressure of a mixture of gases in a container is the sum of the individual pressures (partial.

Chapter 14 Behavior of Gases. I KnowFuzzy Need to Learn I will learn to List and explain the properties of a gas and explain how the kinetic molecular.

A Reminder… assume ideal

QUIZ – WED CASTLE LEARNING / EXAM - FRIDAY

Chapter 14 Gas Behavior.

Warm-Up 12/14/2016 How many moles of nitrogen are in 135 L of nitrogen gas at Standard Temperature and Pressure(STP)? A) 4.82 moles of N2 B) 5.53 moles.

Journal 1)Convert the following pressures to pressures in standard atmospheres: A kPa B. 456 torr Conversions 1 atm=101.3 kPa= 760 mm Hg= 760.

Gas Laws Chapter 14.

Warm Up 7.1 Fluorine 300K occupies a volume of 500mL. To what temperature should it be lowered to bring the volume to 300mL? A sample of hydrogen.

Diffusion and Effusion

Chemistry 14.4.

Chapter 12 Notes, Part II Ideal Gas Law

Density, Dalton Avogadro & Graham

Chemistry 14.4.

Molar Mass and Molar Volume

Chapter 13 The Gas Laws.

Honors Chemistry Chapter 12 Gas Laws.

Chapter 14: The Behavior of Gases

Kinetic Molecular Theory

Gases: Mixtures and Movements

Chapter 11 Gases Four factors that can affect the behavior of a gas.

How does a gas differ from a solid and a liquid?

Chemistry 14.4.

Effusion and Grahams Law, Daltons Law and non Ideal gases

Kinetic Molecular Theory and Gases

Guy-Lussac’s Law P1 / T1 = P2 / T2 Avogadro’s Law V1 / n1 = V2 / n2

Chapter 13 Kinetic Theory (Kinetikos- “Moving”)

Gas Laws The Behavior of matter.

Warm Up #2 For the following problems, label P, V and T as well as the law you are using. You have a container with 2.4 atm of pressure at 340 K. How.

Gases continued.

Chemistry 14.4.

Starter S-146 List five properties of gases..

Avogadro’s Law.

Moles and Gas Volume (3.4) Avogadro’s Hypothesis: equal volumes of different gases at the same temperature and pressure contain the same number of particles.

Gas Laws Chapter 14.

Pre-AP Chemistry, Mr. Guerrero

Combined Gas Law and Dalton’s Partial Pressure Law

Factors that affect gases

Chapter 12 Notes, Part II Ideal Gas Law

Notes Ch Gases: Mixtures and Movements

Bell Ringer (on Friday) 1

Chemistry 14.4.

Presentation transcript:

Warm Up #3 You are given a 5000.0 mL container of SO2 gas with a pressure of 1.4 atm. If the temperature of this gas is at 25oC, how much gas will you have, in grams? You have 4.5 L of a gas at a pressure of 450 mmHg and a temperature of 300 K. How would the volume of the gas be different if it was at STP? You are given a gas with a pressure of 50.4 kPa. If you were to triple the temperature, how would that effect the pressure? Why would this happen?

Diffusion vs. Effusion Diffusion – molecules moving from HIGH to LOW concentration/pressure Effusion – gaseous molecules escaping through small hole in container (high to low pressure)

Graham’s Law Graham’s Law – large, fatty molecules move slower than small, skinny ones M = molar mass 1 = smaller gas 2 = larger gas

Example Problem 1.25 Which gas moves faster, N2 or CO2? By how much? N2 = 28.02 grams (M1) CO2 = 44.01 grams (M2) N2 is lighter, so it will move faster…but by how much? 44.01 28.02 This means N2 will move 1.25x faster than CO2 1.25

Dalton’s Law of Partial Pressures container filled with multiple gasses Pressure of container = pressure of each gas PT = P1 + P2 + P3…

Example Problem A container with four different gasses has a pressure of 160 mmHg. Gas 1 has a pressure of 20 mmHg, Gas 2 has a pressure of 65 mmHg and Gas 3 has a pressure of 40 mmHg. Find the pressure of Gas 4. P4 = PT – P1 – P2 – P3 P4 = 160 – 20 – 65 – 80 = 35 mmHg P4 = 35 mmHg

Quick Quiz #2 Which gas is likely to effuse faster, carbon dioxide or nitrogen gas? Why have you chosen your answer? Show, using Graham’s Law, the difference in speed. You are given a container containing 4 gasses at 340 mmHg of total pressure. One gas is at 0.09 atm, another at 120 mmHg, and another at 13 kPa. How much pressure is exerted by the final gas? You have a gas in a 456 mL container. If the molar mass of this gas is 23 grams per mole, find out how many moles of gas you have at STP conditions. Also, find how many grams of gas you have.

Warm Up #4 You are comparing the rates of two gasses: oxygen and a mystery gas. You find out this mystery gas moves 4 times faster than oxygen. What gas is this? You are given 68.0 g of dinitrogen monoxide gas at 800 K in a 10 L container. How much does this gas exert in mmHg? You have a gas at a constant volume of 50.0 mL. If you change the current STP conditions to 1100 mmHg, how will the temperature be affected?