Chemistry 11 – Mole Concept Study Guide 9

Ideal Gas: 1. John Dalton: (On the right)

Focused on ___________ of gas. E.g., 11.1g of H2 combine with 88.9g of O2 46.7g of N2 reacts with 53.3g of O2 42.9g of C reacts with 57.1g of O2 → No real pattern is observed :(

2. Joseph Gay-Lussac: Focused on __________ of gas. E.g., 1L of H2 combine with 1L of Cl2 to produce 2L of HCl 1L of N2 reacts with 3L of H2 to make 2L of NH3 2L of CO reacts with 1L of O2 to make 2L of CO2 → Gives nice relationship, but he could not explain why…

3. Avogadro: (On the left)

Came up with a hypothesis to explain Joseph’s experimental data: Avogadro’s hypothesis:

1. What does the hypothesis mean?→ Notice how the hypothesis is focused on the __________, not ________. This hypothesis tells us that 2L of gas AB will be made by combining 1L of reactant A and 1L of reactant B. 2. What does the hypothesis mean? → If two gases contains the same number of ___________ and are found under the same ___________ and ___________, both gases occupy the same ___________.

Standard Temperature and Pressure (STP)

Standard Temperature = ___________oC Standard Pressure = ___________kPa

Molar Volume (L/mol) (The ___________ occupied by ___________ mole of the gas.)

The volume of one mole of ANY gas at STP is___________L

Conversion factors: (22.4L/mol is true for only gases!, not liquid or solid)

!!!!!!!!!!!!!!!! or

mass

Volume

Hz t Clz → ZHCI

1 Nz -13H2 → 2 NH 's

2 CO t 102 → 2 CO2A a a

MOI MOI MOI

Equal Volumes of different gasesat the same temperature 4 pressure

contain the same # of particles .

Volumemass

Moles

temperature pressure volume

O = 273.15K

101.3 = I Atm

Molar Mass ( glmol ) The mass occupied by 1 mole of substance

Volume 1

22.4

22.4L I mo )-

-

I MOI 22.4L

Chemistry 11 – Mole Concept Study Guide 10

Eg. How many moles of H2 are there in 10.0L of H2(g) at STP? Road Map: ______ of hydrogen → _______ of hydrogen

Try the harder one: Eg. How many atoms of chlorine are there in 10.0L of chlorine gas at STP? (Hint: Halogens are diatomic elements.) Road Map : ________ of chlorine → ________ of chlorine → ________ of chlorine → ________ of chlorine

When density is mentioned at any point in a problem, you should immediately remember that:

density (g/L) = mass (g) volume (L)

And find a way to get ________ and ________ through ________. (Use the heart of mole to help you get to the mass and volume.) Eg. How many moles are contained in 7.50L of C2H5OH(l)? (density 0.789g/mL) Road Map: Use ________ → ________ → ________

Another useful formula for a problem dealing with density is:

density (g/L) = molar mass (g/mol) molar volume (L/mol)

Note: ________ can be substituted for molar volume if gas is at STP.

DOvolume Mol / I

L

A

" "=

3 SF Imo I

10.04142cg)× = 0.4464285 . . - MOI Hzcg

,

3 SF= 0.446MOI Hug )

Ck Ck CkVolume mot molecule atom

Cl L n a a

MV Av Ra#3 Diggs

DVSTP 6-02 molecular formula10.0L Ck

×A MOI

3×1023MOKEYLK A 2atoms c ,

22.4 L•

I MOI U2as

I molecule Q2

3

23

5. 375 X 10 atoms Cl = 5.38×1023 atoms Cl

Key p . 267 n 268

HF : ReviewQ 161-117 ANI Sto ich

QI - 3 Ckey online )