Classify each of these reactions.

(1) ba(clo3)2(> bacl2(s) + 3o2(g)
(2) 2nacl(aq) + k2s(> na2s(aq) + 2kcl(aq)
(3) cao(s) + co2(> caco3(s)
(4) koh(aq) + agcl(> kcl(aq) + agoh(s)
(5) ba(oh)2(aq) + 2hno2(> ba(no2)2(aq) + 2h2o(l)

each classify reaction should be either one of this.

(a) acid-base neutralization
(b) precipitation
(c) redox
(d) none of the above

1) Redox reaction

2) none of the above

3) none of the above

4) precipitation

5) acid-base neutralization

Explanation:

(1) Ba(ClO3)2(s)--->BaCl2(s) + 3O2(g)

In this reaction a single reactant produces (two or more)products which is a decomposition reaction.

But This is also a redox reaction, because Cl is reduced from

and Oxygen is oxidized . The answer is redox.

(2) 2NaCl(aq) + K2S(aq)--->Na2S(aq) + 2KCl(aq)

This reaction gives no insoluble precipitatwhich means, no reaction, despite the fact that it looks like a double replacement reaction. So the answer is none of the above.

(3) CaO(s) + CO2(g)--->CaCO3(s)

This is a synthesis (or combination) reaction where two or more reactants are formed out of 1 single product. So none of the above.

(4) KOH(aq) + AgCl(aq)>KCl(aq) + AgOH(s)

This is a double decomposition reaction, also called a precipitation reaction, where two soluble salts react to form an insoluble salt and a soluble salt.

(5) Ba(OH)2(aq) + 2HNO2(aq)--->Ba(NO2)2(aq) + 2H2O(l)

An acid and a base react to form water and a salt and involves the combination of H+ ions and OH- ions to generate water.

This is a double replacement or acid/base reaction.

"the periodic table is arranged in order of atomic number."