Name _______________________________
#_____
Honors Chemistry
Carpenito/Dinota
Reading Guide: Stoichiometry
Chapter 9
Section 9.1: Introduction to Stoichiometry AND Section 9.2: Ideal Stoichiometry Calculations
Define the terms:
reaction stoichiometry:
mole ratio:
Review question: What do the coefficients in a balanced chemical equation represent?
Review Question: Why must chemical equations be balanced?
Using the balanced equations below, determine the total number of moles of product formed:
1.
H2CO3(aq) → H2O(l) + CO2(g)
___________
2.
2KClO3(s) → 2KCl(s) + 3O2(g)
___________
3.
Cl2(g) + 2NaBr(aq) → 2NaCl(aq) + Br2
___________
In equation 2 above, how many moles of O2(g)will form if 6 moles of KClO3(s) are decomposed? _________
How is the mole ratio used in stoichiometry problems?
Why is it necessary to convert mass to moles in stoichiometry problems?
Read pages 286-287 carefully to answer the following:
Why does the mass of tin increase when tin is heated in air?
What do you think “phlogiston” was mainly composed of based on the observations of Rutherford and Priestly?
Outline the steps that must be done to determine the grams of water formed by the combustion of 29 grams of butane
in the balanced equation below. Do NOT do the actual calculation…explain the steps you must follow.
2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 1 0H2O(g)
2NaF(l) → 2Na(s) + F2(g)
Calculate the number of grams of sodium and the number of grams of chlorine that form when 112 grams of NaF
decomposes. Show how this illustrates the law of composition of matter.
Use the steps outlined in these sections to determine which reaction below will yield the greatest mass of hydrogen gas
if 20.0 g of each metal (Na or Mg) is reacted with water according to the balanced equations below: (Show all work!)
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Mg(s) + H2O(g) → MgO(s) + H2(g)
Metal that produces the greatest mass of hydrogen__________________
Section 9.3 : Limiting Reactants and Percent Yield
Define the terms:
limiting reactant:
excess reactant:
theoretical yield:
percent yield:
Distinguish between the limiting reactant and excess reactant in a chemical equation.
When a sandwich is made with 2 pieces of bread, 3 slices of meat and 1 slice of cheese, how many sandwiches can be
made with 30 slices of bread, 30 slices of meat and 30 slices of cheese.
What is the limiting reactant above? Why is it limiting when you have the same quantity of each sandwich component?
HOW can you be sure that a stoichiometry question involves a limiting reactant?
N2 (g) + 3H2(g) → 2 NH3(g)
Determine the mass of NH3(g) formed by the reaction of 150 grams of hydrogen gas with 100 grams of nitrogen gas.
(SHOW ALL WORK!!)
Explain why the amount of product formed by the excess reactant would violate the law of composition of matter.
Why are actual yields frequently less than theoretical yields?
In the reaction below, if 58 grams of nitrogen is reacted with 10 grams of hydrogen, what is the theoretical yield of
ammonia? If the reaction yields 60 grams of ammonia, what is the percent yield?
N2 (g) + 3H2(g) → 2 NH3(g)
How much ammonia would be produced above if the percent yield of the above reaction was 90%?