Yes, more math!!. Plan of the Day Review Balancing equations Mass to mass problems Introduce Mass to Volume Equations Introduce Volume to Volume Equations.

Yes, more math!!

Plan of the DayReview

Balancing equationsMass to mass problems

Introduce Mass to Volume EquationsIntroduce Volume to Volume

EquationsHW Time

Plan of the Day 4/15/11Review Molar Volume Lab

RecalculationsReview Ch 10 Test

In groups, work through each problemTake notes as neededQuestions???

Ch 10 Retest next class – best score Current HW Questions???

Plan of the Day 4/18/11Review Molar Volume Lab

RecalculationsReview Ch 10 Test

In groups, work through each problemTake notes as neededQuestions???

Ch 10 Retest next class – best score Current HW Questions???

Plan of the Day 4/20/11Ch 10 Retest Today – for best

scoreAny last minute Questions?

Continue w/ Ch 11 & 12 HWMass/Volume Lab 4/22/11Mass/Volume Lab 4/22/11Chapter 11 & 12 Test 4/26/11Chapter 11 & 12 Test 4/26/11

Plan of the Day 4/21/11Mass/Volume Lab

Conduct, calculate & turn in Continue w/ Ch 11 & 12 HW

Chapter 11 & 12 Test Chapter 11 & 12 Test 4/25/114/25/11

& HW Quiz& HW Quiz

Plan of the Day 4/22/11Mass/Volume Lab

Conduct, calculate & turn in Continue w/ Ch 11 & 12 HW

Ch 11 #1-11 & 15Ch 12 #1-10

Chapter 11 & 12 Test 4/26/11Chapter 11 & 12 Test 4/26/11& HW Quiz& HW Quiz

Balancing EquationsWhat do you remember? (lets just

brainstorm!)What do the balanced equations tell you?Why? Law of Conservation—who can

explain?How do Chemists use this relationship?

Like a recipe! Let’s try one: Ca + H2O Ca(OH)2 +

H2

Ca + 2 H2O Ca(OH)2 + H2

And another : C2H6 + O2 CO2 + H2O2C2H6 + 7O2 4 CO2 + 6 H2O

Balancing EquationsVideo’s?

http://www.youtube.com/watch?v=RnGu3xO2h74&playnext_from=TL&videos=h7PQ10ClYzI

Mass to Mass Example 1 Given a certain amount of a reactant how do

we find the mass of a certain product? 2C2H6 + 7O2 4CO2 + 6 H2O How much ethane would it take to get 20

grams of carbon dioxide? Balance Equation Identify known & unknown Equation to solve

Mass of known to moles of known Moles known to moles unknown Moles unknown to mass unknown Balance

Equation

Mass to Mass Example 2How many grams of glucose form when

88.0 g of CO2 reacts?CO2 + H20 C6H12O6 + 6 O2

First what are the steps? Using words write them down.

Now what purpose does each step serve? Using words!

Share with the class!Calculate Answer is 60.0g C6 H12O6

Mass to Volume… Blue Book Ch. 11

What is the relationship between moles and volume with gases?

How do we get from volume to mass and vice versa?

What are the steps?

Mass to Volume cont..

1. Balance Equation2. Identify known &

unknown3. Mass to Moles (known)4. Moles (known) to

Moles (unknown)5. Moles (unknown) to

Volume of unknown (22.4 dm3 = 1 mole)

Ch 11 Mass to Volume Example 1

Calculate the volume of oxygen produced at STP by the decomposition of 10.0 g of potassium chlorate, KClO3.

KClO3 KCl + O2 Hint

Balance the equationI.D. known & unknownConvert the grams to molesConvert moles of KClO3 to moles of O2Convert moles of oxygen to volume using our handy

22.4 dm3 = 1 mol of any gas @STP!Answer: 2.74 dm3 O2

Ch 11 Mass to Volume Example 2

How many cubic centimeters of hydrogen are produced by the reaction of .750 grams of sodium metal with excess water?

Na + H2O NaOH + H2

HintBalance the equationConvert the sodium to molesConvert moles of sodium to moles of hydrogenConvert moles of hydrogen to volume using our

handy 22.4 L = 1 mol of any gas!Throw in a cm to dm conversion

Answer: 365 cm3

Ch 11 Mass to Volume Example 3Al reacts with HCl to produce aluminum

chloride and hydrogen gas. How many dm3 of hydrogen at STP are produced if Al reacts with an HCl solution which has a mass of 80.0g and contains 70.0% water?

Al + HCl AlCl3 + H2

If 80.0 g of a solution of HCl is 70% water then it is 30% pure HCl, use part to whole:

30g pure HCl/100 g solution of HCLANSWER: 7.36dm3 H2

Ch 11 Mass to Volume Example 4How many grams of ammonium sulfate must

react with excess sodium hydroxide to produce 400 cm3 of ammonia measured at 27oC and 98.0 kPa?(NH4)2SO4 + NaOH Na2SO4 + NH3

+ H2O

Answer: 1.04 g (NH4)2SO4

Ch. 12 Volume to Volume:Ch. 12 Volume to Volume: How do chemists convert volume to volume???First Step?

Balance the EquationSecond Step?

ID known & unknownThird Step

Volume of known to Moles of known

Fourth Step? Moles of known to

moles of unknownNext?

Moles of unknown to volume of unknown.

Volume to Volume Example 4 If 6.00 dm3 of oxygen are available to

burn carbon disulfide, how many dm3 (liters) of carbon dioxide are produced? The products of the combustion of carbon disulfide are carbon dioxide and sulfur dioxide.

CS2 + O2 CO2 + SO2

1. Volume to Mole (known)2. Mole (known) to Mole (unknown)3. Mole (unknown) to Volume (unknown)

2.0 dm3 CO2

Anybody see a shortcut??All gasesSo…

6.00dm3 1 dm3 CO2 3dm3 O2

= 2.oo dm3 CO2

the known volume can be multiplied by the mole ratio to find unknown volume (see p. 120 in Blue Book)

CAREFUL… only if the gases are measured under the same conditions of temperature & pressure

Chapter 12 – example 3When a hydrocarbon such as ethylene burns complete in oxygen, the products are carbon dioxide and water. Calculate the liters of air required to burn completely 15.0 dm3 of ethylene gas, C2H4, measured at STP. Assume that air contains 21.0% oxygen by volume.

C2H4 + O2 CO2 + H2O

*Hint: the answer needs to be stated in dm3 of air – but only oxygen in the air reacts with ethylene gas.

Answer: 214 dm3 of air

Ch 12 Volume to Volume Example 5 How many liters (dm3) of air measured at

98.5 kPa and 100o C are required to produce 200dm 3 of CO2 measured at the same pressure and 20o C? Assume that air contains 21% oxygen by volume and that the CO2 is being produced from CO.

CO + O2 CO2 Balance Equation Old/New Chart to find missing volume Conversions?

1 dm3 O2 = 2 dm3 CO2 21 dm3 O2 = 100 dm3 air

Put it all togetherANSWER: 606 dmANSWER: 606 dm33 airair

Chapter 11 Mass-Volume HWChapter 11 Mass-Volume HW#1-11 & 15#1-11 & 15

Chapter 12 Volume-Volume HWChapter 12 Volume-Volume HW#1-10#1-10*Chapter 11 & 12 Test: 4/19 & 4/20**Chapter 11 & 12 Test: 4/19 & 4/20*

(B-day) (A-(B-day) (A-day)day)