# Stoichiometry initial

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Stoichiometry: Using Balanced Equations
Follow these steps as appropriate for the problems:
A. Balance each equation. Include symbols of state, such as (s), (g), (aq), etc.
B. Determine the number of moles of the given substance.
C. Use the given number of moles to find the requested number of moles.
D. Find the number of grams of the requested substance.
E. Check

I. Synthesis Reactions
1. Strontium + Phosphorus 
Given 50.0 grams of Strontium; find grams of Phosphorus required for complete reaction.

2. Tin + Nitrogen 
Given 12.5 grams of Tin, and more than enough Nitrogen; find grams of Tin (IV) Nitride
produced

II. Decomposition Reactions
3. Aluminum Chlorate       ( forms a metallic chloride and oxygen )
Given 172.0 grams of Aluminum Chlorate; find grams of Oxygen produced, assuming complete
reaction

4. Arsenic (V) Hydroxide ( forms a metallic oxide and water )
Given that 8.5 x 102 g of Arsenic Oxide was produced; find grams of Water also produced.

III. Single Replacement Reactions
5. Potassium Bromide + Chlorine 
Given 45.25 grams of Potassium Bromide; Find grams of Chlorine required for complete
reaction.
p. 2
6. Water + Calcium 
a. Given 4.5 grams of Calcium, and an excess of water; find the theoretical yield of Hydrogen.
b. Suppose that 0.18 grams of Hydrogen were actually produced. What is the % Yield?

IV. Double Replacement Reactions
7. Hydrochloric Acid + Sodium Hydroxide 
a. Given 0.265 grams of Sodium Hydroxide, and excess Hydrochloric Acid; calculate the
theoretical yield of water produced in the neutralization.
b. If only 0.110 grams of water was produced, what was the % yield?

8. Silver (I) Nitrate + Copper (II) Carbonate 
If 40.855 grams of Silver (I) Nitrate completely reacts, what is the theoretical yield of
precipitate?

V. Combustion:

9. Butane combusts.
Given 7.50 x 106 grams of butane completely combust,
a. find the mass of Carbon Dioxide and
b. the mass of Water produced.

10. Methane combusts.
a. Given 3.55 x 104 grams of methane is burned, find the mass of Oxygen required for complete
combustion.
b. Suppose that 2.00x105 g of Oxygen is provided. Which reactant is the limiting reagent?
Which is in excess?

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