For each of the following chemical reactions:

Question

a.)classify the reaction as combination, decomposition,single replacement, or double replacement.
b.)complete the word equation.
c.)using the formulas for both reactants and products, balance the chemical equation.

1. tin(IV)nitrate + magnesium ---> ?
2. potassium oxide + water ---> ?
3. cobalt(III) + lead(II)acetate---> ?
4. aluminum bicarbonate ---^--> ?
5. copper(II)hydroxide + phosphoric acid ---> ?

Answer 1

I will be happy to critique your thinking. Repost with your thinking.

Answer 2

Single replacement. You get magnesium nitrate and tin.
Combination - you get potassium hydroxide.
single replacement - you get cobalt acetate and lead
decomp - you get aluminum, carbon dioxide, and hydrogen gas
double replacement - you get copper phosphate and water

Answer 3

I am just having problems balacing out the reactions.

Answer 4

These look ok to me except for the decomposition of aluminum bicarbonate. First, I can't find aluminum bicarbonate OR aluminum carbonate listed in The Merck Index. Assuming it exists, I would think CO2, H2O, and the metal oxide as the products upon heating.

For balancing, here is the first one.
Sn(NO3)4 + 2Mg ==> 2Mg(NO3)2 + Sn
If you will explain the problem you are having with balancing, perhaps we can help you understand how to do them.

Answer 5

I have:
1.)Sn(NO3)4 + 2Mg----> 2Mg(NO3)2 + Sn

2.)K2O + H20 ----> 2KOH

3.)CO2(SO4)3 + Pb(C2H3O2)2 ----> CO(CH3COO)2 4H20 + Pb

4.)Al(HCO3)3---> AlCO2 + H2

5.)Cu(OH)2 + H3PO4----> Cu3(PO4)2 + H2O

Answer 6

5. copper(II)hydroxide + phosphoric acid ---> double replacement - you get copper phosphate and water

Shouldnt this one be single replacement?

Answer 7

Did I balance them correctly?

Answer 8

I'm just saying i know its like 5 and a half years late but for 4 its:
Al(HCO3)3 ---> Al2(CO3)3 + CO2 + H2O

Answer 9

2Al(HCO3)3 ---> Al2(CO3)3 + H2O + CO2 but this isnt balaced right anyway so