What Type of Reaction Worksheet
NAME______________________
Write the correct skeleton equation for each reaction, then balance by putting in coefficients. Use symbols (aq), (s), (g) etc.
_____1. Solid aluminum oxide reacts with water to produce aqueous aluminum hydroxide.
_____2. Solid lead (IV) oxide decomposes to an element which is solid and an element which is a gas.
_____3. Solid zinc reacts with an aqueous solution of tin (II) chloride to form a different solid and a
different aqueous solution.
_____4. Solid zinc reacts with an aqueous solution of hydrochloric acid to form a gas and a different
aqueous solution.
_____5.Write the equation for the reaction between aqueous solutions of silver nitrate and
magnesium chloride. The silver cation always has a + one charge. Check the solubility table to
determine which product is the precipitate and which remains in aqueous solution.
_____6. Write an equation for the reaction involving gaseous fluorine and aqueous potassium iodide.
Check with the appropriate table to see if this reaction would occur at all and if it does occurs,
remember that a nonmetal would replace another nonmetal. Pure iodine exists as a solid.
_____7. Would the following reaction occur? Aqueous solutions of aluminum hydroxide and
sulfuric acid react to form aqueous aluminum sulfate and water. Yes or No (Circle one)
If it does occur, write the balanced chemical equation:
_____8. Solid silver & gaseous sulfur produce solid silver sulfide. (The silver cation is always a + one charge.)
redox 9. Solid CaC2 reacts with water to form ethyne gas and aqueous calcium hydroxide.
_____10. Ethyne gas (a.k.a. acetylene gas) reacts with oxygen to form two different gases & energy.
Now go back through the reactions and label the type of reaction as S for synthesis,
D for decomposition, Comb for combustion, SR for single replacement or DR for double replacement
WRITE THE CHEMICAL EQUATION FOR EACH REACTION THAT OCCUR AND THEN BALANCE.
_____11. Aqueous solutions of potassium chloride and lead (II) nitrate react to form new products.
Check the solubility table to determine which product is the precipitate and which is the aqueous
solution.
______12. The reaction of an organic compound with oxygen produces what two gases? Complete and
balance the following. (Be careful to count all O-atoms and all H-atoms. It also helps to convert the
first formula to a molecular formula.)
C2H5OH
+ O2
→
_____13. Solid mercury (II) oxide forms liquid mercury and oxygen gas.
_____14. Write the equation for a reaction between gaseous chlorine and aqueous potassium iodide.
Check with the appropriate table to see if this reaction would occur at all and if it does
occurs, remember that a nonmetal would replace another nonmetal.
_____15. Write the balanced chemical equation if there is a reaction between aqueous solutions of
copper (II) nitrate and sodium sulfide. (Use the solubility table.)
_____16. Write the balanced chemical equation if there is a reaction between aluminum metal
& solid iron (III) oxide.
_____17. Solid calcium is thrown into an aqueous solution of HCl. Write the balanced chemical
equation for the reaction only if it occurs.
_____18. Hydrogen gas and aqueous FeO are added together. Write the balanced chemical equation
for the reaction, only if it occurs.
_____19. Write the balanced chemical equation to describe solid carbon and oxygen producing
carbon monoxide gas.
_____19. Will aqueous solutions of aluminum sulfate and sodium hydroxide react? If so, write
the skeleton equation for this reaction and then balance.
Now go back through Reactions #11-19 and label each type: S for synthesis, D for decomposition, Comb for combustion,
SR for single replacement or DR for double replacement or No Rxn in the instances where there was not a reaction.