Stoichiometry Escape Room

Stoichiometry

Breakout

Mr. Gibbs, HVA

You will turn in your work...So, be sure to have out a sheet of notebook paper. Click here to get started

Intro

In this breakout, you will solve stoichiometry problems in order recover the uranium stolen from Mr. G's lab. You will need to write down the numbers you encounter along the way so that you know which locker to look in at the end. Good Luck!

Answer the question and you will discover the direction of the next stage

Calculate how many moles of NO2 form when 15.2 g of N2O5 reacts completely according to the equation2 N2O5 (g) --> 4 NO2 + O2 (g)

0.281 moles

0.182 moles

0.821 moles

Mission 1

Misión 3

Locked

Misión 2

Locked

Misión 4

Locked

The first number of the locker containing the uranium is 2. Write it down!

Mission 2

Misión 3

Completed

Locked

Misión 4

Locked

The next number of the locker is 1.

68 moles

86 moles

34 moles

Consider the balanced equation for the combustion of hexane2C6H14 (g) + 19O2 (g) --> 12CO2 (g) + 14H2O (g) Determine how many moles of O2 are required to react with 7.2 moles of C6H14.

ACDB

BCAD

DACB

Consider the equations below: A: 4N2 + 5O2 --> 2N4O5 B: N2 + 3H2 --> 2NH3C: 3N2 + Ag --> 2AgN3 D: 3N2 + Ba --> BaN6 If you begin with 2.0 moles of Nitrogen gas in each: 1. Determine the #moles of product 2. Put the equations in order from greatest # moles to lowest.

85.2%

35.8%

58.3%

Lead II ions can be removed from solution according to the equationPb2+ (aq) + 2 KCl (aq) --> PbCl2 (s) + 2 K+ (aq) When 18.49 g of KCl is added to a solution containing Pb2+, a precipitate of PbCl2 forms. In the lab the solid PbCl2 is filtered and found to have a mass of 29.4 g. Determine the theoretical yield of PbCl2, and calculate the percent yield of the reaction.

The last number is 6. You're getting close!

Misión 2

Mission 3

Completed

Completed

Misión 4

Locked

Hope you wrote those numbers down...

Answer the question and you will discover the following clue

$80.91

$2291.94

$20.22

If we were to add a piece of solid Cu to an aqueous solution of silver nitrate, the Silver would be replaced in a single replacement reaction forming aqueous copper (II) nitrate and solid silver. Cu (s) + 2 AgNO3 (aq) → Cu(NO3)2 (aq) + 2 Ag (s) What is the theoretical yield of silver produced if 150 grams of Cu is added to the solution of excess silver nitrate? If silver is selling for $4.50/ounce (1 gram = 0.0353 ounces), how much could you make if you sold the silver you collected from this reaction? How much is it worth?

Need a little help? click here

First, calculate the mass of silver (Ag) in grams. To convert grams to ounces, multiply grams times conversion factor (1 g = 0.0535 oz.) Example: 15 grams = _______ oz. 15 x 0.0353 = 0.5295 oz. Lastly you have to multiply the number of ounces times $4.50 ($4.50 per ounce).

Write down the answer to the problem below, you'll need it.

14+3

Misión 2

Misión 3

Completed

Completed

Completed

Mission 4

Enter the number from the last clue multiplied by 3.

Wrong answer!

Try again!

Misión 2

Misión 3

Completed

Completed

Completed

Congratulations you have completed all the missions and retrieved the stolen uranium!1. Submit a screen shot of this screen to Canvas. 2. Turn in your work to Mr. Gibbs

Misión 4

Completed