final exam review, part i get ready for battleship! you need… 1)a calculator 2)a periodic table...

Final Exam Review, Part I

Get ready for Battleship!You need…1)A calculator2)A periodic table (with a back)3)A formula chart4)Your final review5)Any notes you may have6)Scratch paper to do the math on – lots of math.7)Your game face! TAKE THOSE OTHER TEAMS DOWN!8)To sit in groups of 3-4.

Final Exam Review, Part I

Get ready for Battleship!

Set-Up:

Number 1-10 on your piece of paper. Each team member must print their name

next to ONE number only. Don’t let any other team see what your

numbers are! These are your battleships.

The Rules

You gain the ability to take shots at other teams’ battleships by getting questions correct. Questions are worth 1, 2, or 3 shots at the team of your choice.

When one of your battleships is sunk, the person who’s battleship was shot will be rescued by their teammates. THE TEAM ONLY DIES WHEN EVERY MEMBER HAS BEEN SHOT.

Once a team is dead, if they get the next question right, they will come back to life as angry ghosts! Ghosts get double shots for every question they get right.

The Rules: Part II

Winners will be determined by which team has the most LIVING battleships at the end of the class.

All students MUST participate. You show this by making sure everyone’s color appears in the answer.

Sharing pens results in immediate disqualification for that question.

Answers are only accepted if written on the group’s white board!

Battleship: Last Questions?

Let the games begin!

Question 1: for 2 shots

How many formula units are in 3 moles of AlF3?

Question 1: for 2 shots

How many formula units are in 3 moles of AlF3?

3 x (6.02 x 1023) = 1.806 x 1024 formula units

Question 2: for 2 shots

N2 + 3 H2 2NH3

At STP, How many liters of Nitrogen gas, reacting with hydrogen gas, are needed to produce 25 L of ammonia (NH3)?

Question 2: for 2 shots

N2 + 3 H2 2NH3

At STP, How many liters of Nitrogen gas, reacting with hydrogen gas, are needed to produce 25 L of ammonia (NH3)?

25 L NH3 x 1 L N2 = (25/2) = 12.5 L N2

2 L NH3

Question 3: for 1 shot

If you have 205 g of NaOH in 350 mL of water:

How many moles of NaOH do you have?

Question 3: for 1 shot

If you have 205 g of NaOH in 350 mL of water: How many moles of NaOH do you have?

205 g x _1 mol NaOH_ = 5.13 mol NaOH

39.997 g NaOH

Question 4: for 1 shot

If you have 5.13 mol of NaOH in 350 mL of water:

What is the concentration (M) of your solution?

Question 4: for 1 shot

If you have 5.13 mol of NaOH in 350 mL of water: What is the concentration (M) of your solution?

350 mL / 1000 = 0.35 L

M = (5.13 mol/ 0.35 L) = 14.7 M

Question 5: for 2 shots

A sample that contains 4.38 mol of a gas at 15 oC has a pressure of 0.857 atm. What is its volume?

Question 5: for 2 shots

A sample that contains 4.38 mol of a gas at 15 oC has a pressure of 0.857 atm. What is its volume?

15 oC + 273 = 288 K

PV = nRT

(0.857 atm) V = (4.38 mol) (0.0821) (288 k)

V = 103.564 / 0.857 = 120.8 L

Question 6: for 1 shot

If Ms. Park needs to make 2.5 L of 0.6 M hydrobromic acid, how much of 12 M acid would she need?

Question 6: for 1 shot

If Ms. Park needs to make 2.5 L of 0.6 M hydrobromic acid, how much of 12 M acid would she need?

(0.6 M) (2.5 L) = (12 M) V2

V2 = (0.6 x 2.5) / 12 = 0.125 L

Question 7: for 3 shots

2 KOH + H2CO3 2 K2CO3 + 2 H2O

How many grams of water will be produced from the neutralization of KOH with 24.8 g of carbonic acid?

Question 7: for 3 shots

2 KOH + H2CO3 2 K2CO3 + 2 H2O

How many grams of water will be produced from the neutralization of KOH with 24.8 g of carbonic acid?

24.8 g H2CO3 x 1 mol x 2 mol H2O x 18.015 g =

62.025 g 1 mol H2CO3 1 mol H2O

= (24.8 x 2 x 18.015) / 62.025 = 14.4 g H2O

Question 8: for 1 shot

Balance the following reaction!

___Cu2O3 ___Cu + ___O2

Question 8: for 1 shot

Balance the following reaction!

2 Cu2O3 4 Cu + 3 O2

Question 9: for 2 shots

What is the mass (in grams) of 3.7 moles of copper atoms?

Question 9: for 2 shots

What is the mass (in grams) of 3.7 moles of copper atoms?

3.7 mol x 63.546 g/mol = 235.1 grams

Question 10: for 2 shots

Identify ALL of the following compounds that would be insoluble (form precipitates) in water:

(NH4)2S PbCl2 Cs2CO3

Mg(OH)2 HClO CaCrO4

Question 11: for 3 shots

List any 3 (out of the 5) postulates of Kinetic Molecular Theory (KMT).

Question 11: for 3 shots

ANY 3:

1.Gas particles are very small (no volume)

2.Gas particles have elastic collisions (energy conserved)

3.Gas particles do not attract or repel each other

4.Gas particles are always in rapid motion

5.The temperature of a gas is directly related to the amount of kinetic energy of the particles

Question 12: for 2 shots

What volume is occupied by 15 moles of CO2 gas at STP?

Question 12: for 2 shots

What volume is occupied by 15 moles of CO2 gas at STP?

15 mol x 22.4 L/mol = 336 L CO2

Question 13: for 2 shots

Write and balance the following reaction:

Phosphorus pentachloride decomposes to yield phosphorus trichloride and chlorine gas

Question 13: for 2 shots

Write and balance the following reaction:

Phosphorus pentachloride decomposes to yield phosphorus trichloride and chlorine gas

PCl5 PCl3 + Cl2