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# I’m hiring! - PowerPoint PPT Presentation

I’m hiring!. Homework Graders Pay = 1 extra credit point/10 papers graded Qualifications : No TUs, BD, LD Availability before/after school or 5 th period lunch. No nepotism/cronyism will be tolerated. HOMEWORK DUE MIErCOLES. If you haven’t done so already, read chapter 3!

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• Pay = 1 extra credit point/10 papers graded

• Qualifications:

• No TUs, BD, LD

• Availability before/after school or 5th period lunch.

• No nepotism/cronyism will be tolerated

• If you haven’t done so already, read chapter 3!

• P114 - 115: #22, #32, #34

The quantitative study of chemical reactions

How much product will form from a given amount of reactants?

How much of the reactants is necessary to form a given amount of product?

• Predict products of a reaction if they are not given to you

• Balance the coefficients of the reaction

• Use molar conversion to change whatever is given (volume, mass or concentration) to moles

• Use the molar ratio from the balanced reaction to convert the moles of what is given to the moles of what’s asked for.

• Use conversion factors (moles  mass, volume or M) to change the moles of what is asked for to the proper unit

Calculate the volume of NH3 formed at STP when 5.0 kg of H2 react with excess N2 to form NH3

Calculate the mass of solid product formed when 18.4 g of MgBr2 is combined with a solution containing excess K2CO3.

• The reactant that gets used up

• The reactant that determines the amount of product formed

Excess Reactant MgBr

• The reactant that Does Not get used up

 You must figure out which one is limiting

3A + 2B MgBr A3B2Which reactant is limiting?

• Do Step 1 and then Step 2 for both A & B.

• Use the molar ratio that relates A to B to determine how much of B would be needed to completely use up the moles of A

• If there are more than enough moles of B, A is limiting

• If there not enough moles of B, then B is limiting

• Use limiting reactant for steps 3 & 4

Calculate the mass of glucose (C MgBr6H12O6) formed when 880 g of carbon dioxide is combined with 720 g of water in photosynthesis

Calculate the mass of BaSO MgBr4 formed when 104 g of BaCl2 is combined with 250 mL 1.00 M K2SO4

2 LL

(lettuce

leaves)

5 BS

(bacon

slices)

3 TS

(tomato

slices)

2 PB

(pieces

+

+

+

So reaction is: MgBr

• 2 PB + 3 TS + 5 BS + 2 LL  1 BLT

1 BLT

• 1 PB = 50.0 g

• 1 TS = 60.0 g

• 1 BS = 20.0 g

• 1 LL = 5.0 g

• 1 BLT = 390.0 g

How many BLTs? MgBr

• PB = 3,356.7 g

• TS = 4,789.2 g

• BS = 2,789.4 g

• LL = 789.2 g

Get answer in significant digits and then round down to whole number of BLTs.

• The amount determined through stoichiometry

• The amount solved for on paper

• The amount obtained in the lab

• Actual yield

Percent yield MgBr

• % Yield = (Exp/Theo) x 100 %

68 g NH MgBr3 was obtained when 140 g of N2 reacts with excess H2. Calculate percent yield.

510 g PH MgBr3 was obtained when 0.62 kg of P4 reacts with excess H2. Calculate percent yield.

4.61 g of lead(II)iodide was obtained when 66.2 g of lead(II)nitrate was added to 750 ml 0.10 M potassium iodide. Calculate the % yield.

Determine the volume of NH 12 kg of erythrose (C3 formed at STP when 2.0 x 1027 molecules N2 reacts with 4.0 kg of H2:

Determine the volume of O 12 kg of erythrose (C2 released at STP when 32 kg of Fe2O3 is purified making

Fe & O2

Calculate the mass of solid product formed when 41.6 g of barium chloride is added to 250 ml of 0.40 M potassium sulfate giving a 50.0 % yield:

Calculate the mass of solid product formed when 2.00 g of calcium bromide is added to 250 ml of 0.40 M sodium sulfate: