Warm-up I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm. If by increasing the temperature to 225.

Slides:

Advertisements

Similar presentations

Ideal Gas Law. Ideal vs. Real Gases Ideal gases obey every law perfectly – They have fully elastic collisions – They lose no energy as they move and collide.

Advertisements

Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you.

Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you.

Gas Laws Mr. Gates Created by Educational Technology Network

Chapter 10 Gases No…not that kind of gas. Kinetic Molecular Theory of Gases Kinetic Molecular Theory of Gases – Based on the assumption that gas molecules.

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

Section 1.3.  Limiting reactant  Excess reactant  Yields:  Theoretical yield  Percentage yield  Experimental yield  Avogadro’s law  Molar volume.

Gas Stoichiometry Section 7.3 pg Gas Stoichiometry Many chemical reactions involve gases as a reactant or a product Gas Stoichiometry – the procedure.

 Slides 3-8 Slides 3-8 ◦ Part One: Kinetic Molecular Theory and Introduction to Gas Laws  Slides Slides ◦ Part Two: Boyle’s Law, Charles’

Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you.

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.

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 12 Gas Laws.

Gas Laws. Properties of Gases 1. Fluids 2. Low density 3. Highly compressible 4. Completely fill a container and exert pressure in all directions.

Unit 10 Gas Laws. I. Kinetic Theory Particles in an ideal gas… 1.gases are hard, small, spherical particles 2.don’t attract or repel each other. 3.are.

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

GAS LAWS Chapter 10.

Behavior of Gas Molecules

Gas Laws Practice Problems 1) Work out each problem on scratch paper. 2) Click ANSWER to check your answer. 3) Click NEXT to go on to the next problem.

GASES and the Kinetic Molecular Theory A.Gas particles DO NOT attract or repel each other B.Gas particles are much smaller than the distances between them.

Gas Laws and Gas Stoichiometry. Kinetic –Molecular Theory Particles of matter (solid, liquid, or gas) are always in motion. This motion has consequences.

Unit 12: Gas Laws. The Kinetic Theory of Gases Gases aren’t attracted or repelled by each other. Gas particles are super tiny, but the space between each.

TEKS 9A: Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as described by Boyle’s law,

Warm-up Make sure you’re ready for today’s quiz! How much heat is required to raise 25 grams of ice at -15 °C to steam at 118 °C? If I raise the temperature.

MOLAR VOLUME. molar volume What is the volume of a gas at STP, if it contains 10.4 moles? What is the volume of carbon dioxide gas (STP) if the.

Gas Stoichiometry. Equal volumes of gases at the same temperature and pressure contain equal amounts of particles The coefficients in a balanced equation.

b The good news is that you don’t have to remember all three gas laws! Since they are all related to each other, we can combine them into a single equation.

JEOPARDY REVIEW The Gas Laws.

Chapter 6 Gases. Kinetic Molecular Theory of Gases Small particles moving continually and randomly with rapid velocities in straight lines Attractive.

Gases Ch.10 and 11. Kinetic-Molecular Theory 1.Gases consist of very small particles that are far apart Most particles are molecules Volume of particles.

What is the combined gas law? What do each of the variables stand for? What units do the variables need to be in? HINT: Check in your notes from Friday!

PHYSICAL CHARACTERISTICS OF GASES Or GAS LAWS KINETIC MOLECULAR THEORY 1. Ideal gases vs. Real gases 2. Perfect elasticity 3. Average kinetic energy.

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

Note: You must memorize STP and the gas laws!!. The Kinetic Molecular Theory states that gas particles are ____________ and are separated from one another.

1.Use the Ideal Gas Law to solve a gas stoichiometry problem.

Chapter 11 – Ideal Gas Law and Gas Stoichiometry.

Warm-up 2H 2 (g) + O 2 (g)  2H 2 O (g) How many liters of water will be produced from 300 grams of Oxygen gas if Hydrogen gas is in excess? (at STP)

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

Kinetic-Molecular Theory and Gas Laws Kinetic-Molecular Theory and Gas Laws.

Bell Work 1.Convert 15.3 atm to kPa 2.Convert 96.3 L of a gas at STP to moles. 3.What is the temperature and pressure at STP? 4.A scientist is trying to.

Unit 9 Review Gases. The Game Board

Gas Laws Kelley Kuhn. Gas Laws! Everybody knows the basics about gases: they are the least dense state of matter, they expand to fill any container in.

Gases. Kinetic Theory of Gases Explains Gas behavior: 4 parts: 1) Gas particles do not attract or repel each other (no I.M. forces).

Chapter 11: Gases. Section 1: Gases and Pressure.

Do Now & Announcements Turn in SOL Review Packet Take out handout from Friday Unit 10 Test THURS 12/18 (open note) Bring in Baby Food/Small Mason Jars.

Can’t directly measure moles Measure units related to moles: –Mass (molar mass) –Number of particles (6.02 x ) –Liters of gas (22.4 Liters at STP)

Today’s Do Now 1/23/15 At what temperature will a 1.0-g sample of neon gas exert a pressure of 500. torr in a 5.0-L container?

 The kinetic theory assumes the following concepts about gasses are true:  Gas particles do not attract or repel each other  Gas particles are much.

The Gas Laws Ch. 14- Gases. Boyle’s Law P V PV = k Pressure and Volume are inversely proportional. As Volume increased, pressure decreases.

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.

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

Ideal Gas Law & Gas Stoichiometry Work out each problem in the 3-step format. Gases notes #4 - Ideal Gas Law & Gas Stoichiometry.pptx.

Gases Boyle’s Law. As the volume of a gas increases, the pressure decreases. –Temperature remains constant.

Gas Laws Review.

 If I have an unknown quantity of N 2 held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams.

Gas Laws Kinetic Theory assumptions Gas particles do not attract or repel Small particles in constant random motion Elastic collisions All gases have the.

The Ideal Gas Law & Co..

Warm-up #6 2. The balloon in the previous problem will burst if its volume reaches L. Given the initial conditions specified in that problem, determine.

Gases Ideal Gas Law.

Gas Stoichiometry At STP

Ideal Gas Law PV=nRT.

Gas Volumes and the Ideal Gas Law

Unit IV – Chapter 7 Section 7.3

No, it’s not related to R2D2

Presentation transcript:

Warm-up I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60 atm. If by increasing the temperature to 225 K and decreasing the pressure to 30 atm causes the volume of the gas to be 29 liters, how many liters of gas did I start with?

The Ideal Gas Law Unit 8, Day 7 Kimrey 4 December 2012

A Bit More About Gases Remember gases are really tiny particles bouncing off of everything. These collisions are perfectly elastic. Meaning that no energy is lost as they collide. It’s because of this that the combined gas law works (P 1 V 1 /T 1 = P 2 V 2 /T 2 ).

Adding more gas So what happens if we add more of a gas? This can be accounted for by the ideal gas law.

Ideal Gas Law PV=nRT P= Pressure V= Volume n= moles R= gas constant T= Temperature

Units Temperature must be in Kelvin. Volume must be in liters (Remember: King Henry Died by drinking chocolate milk) Pressure can be in atm, mmHg, or kPa BUT you must use the appropriate R for whatever units of pressure you have. R is a constant and can be: (three options are found on the reference tables)

Converting to Kelvin Temperature can also be measured in a unit known as Kelvin. ▫Degrees Celsius plus 273 = Temperature in Kelvin ▫You don’t have to remember this! The reference tables show that 0 °C is the same as 273K 45°C is what in Kelvin? 5°C is what in Kelvin?

Example How many moles of a gas at 100°C does it take to fill a 1.00L flask to a pressure of 1.50 atm?

Example If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?

Example If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, how many atmospheres of pressure are inside the container?

Example If I have an unknown quantity of N 2 held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams of N 2 do I have?

Warm-up If I have an unknown quantity of N 2 held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many grams of N 2 do I have?

Stoichiometry!! Unit 8, Day 7 Kimrey 4 December 2012

Molar Volume 1 mole = 22.4 L of a gas at STP STP = 0°C and 1 atm

Examples How many liters of Nitrogen gas are there in 4.56 moles? How many liters of fluorine are there in 56.7 grams?

Stoichiometry…Again! N 2 + H 2  NH L of nitrogen will produce how many liters of ammonia (at STP)? Don’t forget to balance!!!

Mole - Volume 2H 2 + O 2  2H 2 O How many liters of water will be produced from 15 moles of oxygen?

Mass - Volume 2H 2 + O 2  2H 2 O How many liters of water will be produced from 100 grams of Hydrogen gas if Oxygen gas is in excess?

STP Standard Temperature and Pressure 1 atm and 0 °C

Example In a laboratory experiment, 85.3 moles of a gas are collected at 24 °C and 733 mm Hg pressure. Find the volume at STP.

Not at STP… Use the ideal gas law to determine volume Then use that volume to complete the stoichiometry

Example Na 3 PO KOH  3 NaOH + K 3 PO 4 If you have 25 moles of KOH at 175 K and 3.4 atm, how many liters of K 3 PO 4 are produced?

Example C 3 H 6 O + 4 O 2  3 CO H 2 O At 823 mmHg and 329 K, 135 moles of oxygen are mixed with excess C 3 H 6 O. How many liters of water are produced?