Download Notes for 4/10 - review for exam on 4/11

Notes for 4/8 review for exam on 4/10
1. Writing balanced equations from word equations
A] barium + nitrogen makes barium nitride
B] iron + iodine yields iron (III) iodide
C] hydrochloric acid + barium hydroxide yields water and barium chloride
D] ammonia decomposes into nitrogen and hydrogen
2. Stoichimetry conversions:
A] How many moles are contained in 5.90 g of carbon?
B] How many moles are contained in 90.0 atoms of silver?
C] How many moles are contained in 2.50 x 1020 molecules of sulfur trioxide?
D] How many moles are contained in 22.0 g of carbon dioxide?
E] How many moles are contained in 12.0 mL of iron. The density of iron is 7.87 g/mL
F] If 3.01 x 1023 atoms has a mass of 32.5 g, what is the molar mass of the material?
G] What is the molar mass of: i) iron (III) acetate ii) disulfur pentaoxide
H] What is the mass of 4.50 moles of krypton?
I] What is the mass of 2.80 moles of copper (II) sulfate?
J] What is the mass of 1 atom of sulfur?
K] What is the mass of 4.70 x 1022 molecules of carbon dioxide?
L] Find the number of atoms in 22.0 grams of disulfur trioxide.
M] Find the number of atoms in 15.0 grams of octane, C8H18.
N] Find the number of molecules in 67.0 grams of calcium carbonate
3. Chapter 5 review
A] What two things do the coefficients in a balanced chemical equation represent? Why can’t coefficients represent the
number of grams that react or are produced? What is molar mass?
B] Given the unbalanced reaction: NH3 + O2  NO2 +
H2O
i) How many moles of oxygen react with 0.055 moles of ammonia?
ii) How many moles of water are produced if 5.00 moles of oxygen react with excess ammonia?
iii) How many moles of nitrogen dioxide are produced if 10.0 grams of ammonia react with excess oxygen?
iv) What mass of oxygen will react with 0.00789 moles of ammonia?
v) What mass of nitrogen dioxide forms if I react 22.0 grams of oxygen with excess ammonia?
vi) If 5.0 g of ammonia react with 29 grams of oxygen, what is the mass of water that will form? What is the LR?
C] Given the unbalanced reaction: V + F2 
VF5 ; If 10.0 g of vanadium react with 17.0 g of fluorine, find the LR,
the mass of product, and the mass of excess reactant.
D] Given the unbalanced reaction: C3H8 + O2  CO2 + H2O ; if 2.70 g of C3H8 reacts with 8.00 g of oxygen, find the
LR, mass of excess, mass of carbon dioxide produced, and the percent yield if 6.00 g of CO 2 is recovered.