II. Gas Stoichiometry. 1 mol of a gas=___ L at STP A. Molar Volume at STP S tandard T emperature & P...

II. Gas StoichiometryII. Gas Stoichiometry

1 mol of a gas=___ Lat STP

A. Molar Volume at STPA. Molar Volume at STPA. Molar Volume at STPA. Molar Volume at STP

Standard Temperature & Pressure0°C and 1 atm

A. Molar Volume at STPA. Molar Volume at STPA. Molar Volume at STPA. Molar Volume at STP

Molar Mass(g/mol)

6.02 1023

particles/molMOLES

Molar Volume (22.4 L/mol)

Molarity (mol/L)

B. Gas Stoichiometry B. Gas Stoichiometry ProblemProblemB. Gas Stoichiometry B. Gas Stoichiometry ProblemProblem

How many grams of CaCO3 are req’d to

produce 9.00 L of CO2 at STP?

CaCO3 CaO + CO2 ? g 9.00 L

A. Limiting ReactantsA. Limiting ReactantsA. Limiting ReactantsA. Limiting Reactants

Limiting ReactantLimiting Reactant• _______in a reaction• determines the amount of _______

Excess ReactantExcess Reactant• added to ensure that the other

______ is completely used up• cheaper & easier to recycle


Available IngredientsAvailable Ingredients• 4 slices of bread• 1 jar of peanut butter• 1/2 jar of jelly

Limiting ReactantLimiting Reactant• _______

Excess ReactantsExcess Reactants• _______________


1. Write a _______ equation.

2. For each ______, calculate the

amount of ________ formed.

3. Smaller answer indicates:

• _____________

• amount of product


79.1 g of zinc react with 0.90 L of 2.5M HCl. Identify the limiting and excess reactants. How many liters of hydrogen are formed at STP?

Zn + 2HCl ZnCl2 + H2 79.1 g ? L0.90 L

2.5M


Zn + 2HCl ZnCl2 + H2 79.1 g ? L0.90 L

2.5M


Zn: 27.1 L H2 HCl: 25 L H2

Limiting reactant: ____

Excess reactant: _____

Product Formed: ______

left over zinc

B. Percent Yield(pp 256-B. Percent Yield(pp 256-258)258)B. Percent Yield(pp 256-B. Percent Yield(pp 256-258)258)

100yield ltheoretica

yield actualyield %

________________________

_________________________

B. Percent YieldB. Percent YieldB. Percent YieldB. Percent Yield

When 45.8 g of K2CO3 react with excess

HCl, 46.3 g of KCl are formed. Calculate the theoretical and % yields of KCl.

K2CO3 + 2HCl 2KCl + H2O + CO2 45.8 g ? g

actual: 46.3 g


K2CO3 + 2HCl 2KCl + H2O + CO2 45.8 g ? g

actual: 46.3 g

Theoretical Yield:


Theoretical Yield = 49.4 g KCl

% Yield = 100 =____%

K2CO3 + 2HCl 2KCl + H2O + CO2 45.8 g 49.4 g

actual: 46.3 g

II. Gas Stoichiometry. 1 mol of a gas=___ L at STP A. Molar Volume at STP S tandard T emperature & P...

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