Download Name__________________________ Period_______ Word

Name__________________________ Period_______
Word EQUATIONS with Reaction Conditions
Problem Set 4
Chemical formulas are used to represent the products and reactants in a reaction. Equations can also contain
much more information. Conditions under which a reaction occurs are often found above the arrow. An
example of a reaction condition is the heat symbol (∆ ), which indicates that the reactants were heated. An
equation can also indicate the physical state of the reactants and products. The physical states of matter
symbols are listed below.
I. Reaction Conditions & Physical States are shown in Equations
 (→) – this arrow indicates that substances have reacted together (can be read as “reacts to yield”,





“yields”, “produces” or “forms”)
∆
(→) – this arrow indicated that the reactants are heated
(s) – solid… all precipitates, powders, crystals or ashes are solids
(l) – liquid…water is in the liquid state unless otherwise indicated)
(g) – gas… all diatomic molecules are gases (H2, N2, F2, Cl2, Br2, Cl2, I2)
(aq) – in aqueous solution (dissolved in water)… all acids are in aqueous state
Part I: Directions
Write a balanced chemical equation to represent each of the following chemical reactions. Replace the
appropriate reaction conditions in the equation. (Don’t forget your diatomic molecules)
1. Iron (solid) + sulfur (solid) when heated → iron (II) sulfide (solid)
2. Zinc (solid) + copper(II) sulfate (in solution) → zinc sulfate (in solution) + copper (solid)
3. Silver nitrate (in solution) + sodium bromide (in solution) → sodium nitrate (in solution) + silver
bromide (in solution)
4. Potassium chlorate (solid) when heated → potassium chloride (solid) + oxygen (gas)
5. Water (with electricity added) → hydrogen (gas) + oxygen (gas)
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Part II: Directions
Write a balanced chemical equation, including the reaction conditions, to represent each of the following
chemical reactions. (Don’t forget your diatomic molecules)
6. Mercury(II) oxide in solution when heated yields liquid mercury and oxygen gas.
7. Liquid sodium peroxide reacts with water and produces a sodium hydroxide precipitate and oxygen
gas.
8. Carbon dioxide gas is mixed with water to form carbonic acid, which is then used in the process of
respiration in humans.
9. Solid white phosphorus is exposed to oxygen gas and results in crystallized diphosphorus pentoxide.
10. Methyl alcohol, CH3OH, is a clean-burning fuel. This alcohol can be made by reacting carbon
monoxide gas and hydrogen gas.
11. A solution of potassium iodide is mixed with a solution of lead(II)nitrate to form a solution of
potassium nitrate and a bright yellow precipitate named lead(II) iodide.
12. Hydrochloric acid is added to liquid ammonia (NH3) to produce the salt ammonium chloride.
13. Lithium hydroxide pellets are added to a solution of sulfuric acid resulting in lithium sulfate crystals
and water.
14. If copper coil is placed into a solution of silver nitrate, silver crystals form on the surface of the
copper. Additionally, highly soluble copper (I) nitrate is generated.
15. When crystalline C6H12O6 is burned in oxygen, carbon dioxide and water vapor are formed.
16. Calcium oxide is an ingredient in cement mixes. When water is added to solid calcium oxide, a
powder, calcium hydroxide, forms.
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