Oxygen is 101 kPa; hydrogen is 505 kPa

Slides:

Advertisements

Similar presentations

Gas Laws Chapters

Advertisements

Section 12.2: Chemical Calculations

Section 12.2: Chemical Calculations

GASES Chapter 5.

Properties of Gases.

The Gas Laws Chemistry Dr. May Gaseous Matter Indefinite volume and no fixed shape Indefinite volume and no fixed shape Particles move independently.

Mole concept applied to gases

Page 3 Kinetic Molecular Theory Is a theory that demonstrates how gases should behave. It is also called Ideal Gas Laws.

Ch. 12 Behavior of Gases. Gases Gases expand to fill its container, unlike solids or liquids Easily compressible: measure of how much the volume of matter.

The Gas Laws Chapter 14 Chemistry.

Year 10 C Pathway Mr. D. Patterson. Outcomes Convert from moles to volume of a gas (and vice versa) at standard temperature and pressure Use the conversion.

For an ideal gas, molarity is directly proportional to pressure M = P

Chapter 12: Stoichiometry

Reading for Tuesday: Chapter Reading for Tuesday: Chapter Homework 11.1 – Due Tuesday 4/14/15 Homework 11.1 – Due Tuesday 4/14/15 Chapter.

Gas Laws Mr. Gates Created by Educational Technology Network

Molecular Composition of Gases Volume-Mass Relationships of Gases.

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.

Energy and Gases Kinetic energy: is the energy of motion. Potential Energy: energy of Position or stored energy Exothermic –energy is released by the substance.

Gases Chapter – The Gas Laws Kinetic Theory = assumes that gas particles:  do not repel or attract each other  are much smaller than the distances.

Kinetic Molecular Theory & Gas Laws. Kinetic Theory of Gases  Gases exert pressure because their particles frequently collide with the walls of their.

Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass.

Mullis1 Gay Lussac’s law of combining volumes of gases When gases combine, they combine in simple whole number ratios. These simple numbers are the coefficients.

Gas Notes I. Let’s look at some of the Nature of Gases: 1. Expansion – gases do NOT have a definite shape or volume. 2. Fluidity – gas particles glide.

Marker Board Review You should have a marker board, a marker, and a paper towel to erase! Ready??? GO!!!

GAS LAWS. Behavior of Gases Gases can expand to fill their container Gases can be compressed –Because of the space between gas particles Compressibility:

Learning about the special behavior of gases

Ch. 12 Behavior of Gases. Gases Gases expand to fill its container, unlike solids or liquids Easily compressible: measure of how much the volume of matter.

STAAR Ladder to Success Rung 4. Boyle’s Law The pressure and volume of a gas are inversely related – at constant mass & temp P 1 V 1 = P 2 V 2.

Gas Laws. The Gas Laws Describe HOW gases behave. Can be predicted by the The Kinetic Theory.

What affects the behavior of a gas? u The number of particles present u Volume (the size of the container) u Temperature 2.

Kinetic Theory and a Model for Gases Particles of gases are small and have insignificant volume. Particles move rapidly and randomly. All collisions are.

Ideal Gases Obey the Laws! The effect of adding gas u When we blow up a balloon we are adding gas molecules. u Doubling the the number of gas particles.

Ideal gases and molar volume

Combine This. Ideally That law on the beach ball Stoichiometry

Chapter 13: Gases. What Are Gases? Gases have mass Gases have mass Much less compared to liquids and solids Much less compared to liquids and solids.

Gases. I.Real Gases (we will not study these much) A. Do NOT apply the Kinetic Molecular Theory 1. The particles in a real gas can NOT be thought of as.

Gas Notes I. Let’s look at some of the Nature of Gases: 1. Expansion – gases do NOT have a definite shape or volume. 2. Fluidity – gas particles glide.

Gases I. What is a gas? There are 3 common states of matter: Solid, Liquid, Gas Solid - Has a fixed shape and volume - Not compressible (molecules tightly.

Gas Laws Test Gas Pressure Gas Pressure Kinetic Molecular Theory of Ideal Gases Kinetic Molecular Theory of Ideal Gases Boyle’s Law (Problems & KMT) Boyle’s.

Gas Stoichiometry!. equal volumes of gases at the same temperature & pressure contain equal numbers of particles equal volumes of gases at the same temperature.

Chapter 14-3 I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H 2 + Cl 2 → 2HCl 1 vol. 1 vol. 2 vol.

Chapter 14-3 I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H 2 + Cl 2 → 2HCl 1 vol. 1 vol. 2 vol.

The Gas Laws u The gas laws describe HOW gases behave. u They can be predicted by theory. u The amount of change can be calculated with mathematical.

Gas Laws. 2 Kinetic – Molecular Theory 1. Particle size – Gases contain _________________________ ______________________________________ – Because so.

NOTES: Gases, Molar Volume, & Stoichiometry – a REVIEW!

Ch. 14 The Behavior of Gases PROPERTIES OF GASES.

Gas Laws. 1. Kinetic Molecular Theory Ideal Gases :  Gas particles do not attract or repel each other.  Gas particles are much smaller than the distances.

Aim: What are the properties of Gases? DO NOW: Fill in the blanks. (increase or decrease for each blank) 1. As the volume of a gas ____________, the pressure.

Gas Team Review Game. ?1 List all 5 parts of the Kinetic Molecular Theory. List all 5 parts of the Kinetic Molecular Theory.

1. 2 Partial Pressure Pressure of individual gases in a mixture.

Gas volumes and moles PAGE 87 OF INB. Essential Question:  How can 2 liters of Hydrogen react with 1 liter of Oxygen and only produce 2 liters of gas?

Gases. Pressure Pressure is defined as the force applied over a given area. Barometric pressure is given on weather reports and is typically reported.

The Property of Gases – Kinetic Molecular Theory explains why gases behave as they do

Chapter 12: Stoichiometry

The Behavior of Gases Chapter 14. Chapter 14: Terms to Know Compressibility Boyle’s law Charles’s law Gay-Lussac’s law Combined gas law Ideal gas constant.

Gases. The Nature of Gases  1. Gases have mass –A car tire weighs more with air in it than it would completely empty.  2. It is easy to compress a gas.

The Gas Laws. As P (h) increases V decreases Apparatus for Studying the Relationship Between Pressure and Volume of a Gas.

PERFORMANCE OBJECTIVES Predict, write, and balance chemical equations Recognize types of reactions Use the Kinetic Molecular Theory explain the relationship.

Gas Laws. Phases of Matter SOLID Definite Shape Definite Volume LIQUID Shape varies depending on container Definite Volume GAS Takes on the shape and.

What are the standard conditions (STP) for temperature and pressure?

The Ideal Gas Law.

Oxygen is 101 kPa; hydrogen is 505 kPa

Presentation transcript:

Oxygen is 101 kPa; hydrogen is 505 kPa All the oxygen gas from a 10.0-L container at a pressure of 202 kPa is added to a 20.0-L container of hydrogen at a pressure of 505 kPa. After the transfer, what are the partial pressures of oxygen and hydrogen? Oxygen is 101 kPa; hydrogen is 505 kPa Oxygen is 202 kPa; hydrogen is 505 kPa Oxygen is 101 kPa; hydrogen is 253 kPa Oxygen is 202 kPa; hydrogen is 253 kPa

Nitrogen monoxide and oxygen gas combine to form the brown gas nitrogen dioxide, which contributes to photochemical smog. How many liters of nitrogen dioxide are produced when 34 L of oxygen reacts with an excess of nitrogen monoxide? Assume conditions of STP. 34 L O2 x 1 mol O2 x 2 mol NO2 x 22.4 L NO2 = 22.4 L O2 1 mol O2 1 mol NO2 = 68 L NO2 3.0 L NO2 138 L NO2 68 L NO2 22.4 L NO2 2 NO2 (g) + O2 (g) → NO2 (g)

trigonal pyramid P4 (s) + 6H2 (g) → 4PH3 (g) 0.42 L PH3 0.28 L PH3 Phosphorus and hydrogen can be combined to form phosphine. How many liters of phosphine are formed when 0.42 L of hydrogen reacts with phosphorus at STP? P4 (s) + 6H2 (g) → 4PH3 (g) trigonal pyramid 0.42 L PH3 0.28 L PH3 1.68 L PH3 22.4 L PH3

Which of the following is not characteristic of matter in the gaseous state? Gases fill their containers completely. The collisions particles undergo with the container walls exert pressure. Gases have mass. The pressure of a gas is independent of its temperature. Gases are compressible. The distances between gas particles is relatively large.

False ... just the opposite! Gases behave most ideally at high pressures and low temperatures.

Which of the following changes would increase the pressure of a gas in a closed container? I. Part of the gas is removed. II. The container size is decreased. III. Temperature is increased. I & II only II & III only I & III only I, II & III none of the above

Which of the following changes would increase the pressure of a gas in a closed container? I. Part of the gas is removed. II. The container size is decreased. III. Temperature is increased. I & II only II & III only I & III only I, II & III none of the above