Classify each of these reactions. Ba ( ClO 3 ) 2 ( s ) ⟶ BaCl 2 ( s ) + 3 O 2 ( g ) acid–base neutralization precipitation redox none of the above 2 NaCl ( aq ) + K 2 S ( aq ) ⟶ Na 2 S ( aq ) + 2 KCl ( aq ) acid–base neutralization precipitation redox none of the above CaO ( s ) + CO 2 ( g ) ⟶ CaCO 3 ( s ) acid–base neutralization precipitation redox none of the above KOH ( aq ) + AgNO 3 ( aq ) ⟶ KNO 3 ( aq ) + AgOH ( s ) acid–base neutralization precipitation redox none of the above Ba ( OH ) 2 ( aq ) + 2 HNO 2 ( aq ) ⟶ Ba ( NO 2 ) 2 ( aq ) + 2 H 2 O ( l ) acid–base neutralization precipitation redox none of the above

Ba(ClO₃)₂ (s) ⟶ BaCl₂(s) + 3O₂ (g)   REDOX

2 NaCl (aq) + K₂S (aq) ⟶ Na₂S (aq) + 2 KCl (aq)        NONE

CaO (s) + CO₂ (g) ⟶ CaCO₃(s) NONE

KOH (aq) + AgNO₃(aq) ⟶ KNO₃(aq) + AgOH (s)  PRECIPITATION

Ba (OH)₂(aq) + 2 HNO₂(aq) ⟶ Ba (NO₂)₂(aq) + 2 H₂O (l)  NEUTRALIZATION

Explanation:

Redox reaction involves the oxidation states. The oxidation state from an element decreases and the oxidation state from other element increases.

It is called redox because one element reduces and the other oxidizes.

Neutralization reaction occurs when an acid and a base react, to produce water an a determined salt.

Precipitation reaction can be produced when a solid is formed as the reactants react.

Ba(ClO₃)₂ (s) ⟶ BaCl₂(s) + 3O₂ (g)   REDOX

Cl changes the oxidation state from 5 to -1  (reduction)

O changes the oxidation state from -2 to 0 (oxidation)

2 NaCl (aq) + K₂S (aq) ⟶ Na₂S (aq) + 2 KCl (aq)        NONE

CaO (s) + CO₂ (g) ⟶ CaCO₃(s) NONE

KOH (aq) + AgNO₃(aq) ⟶ KNO₃(aq) + AgOH (s)  PRECIPITATION

Ba (OH)₂(aq) + 2 HNO₂( aq ) ⟶ Ba (NO₂)₂(aq) + 2 H₂O (l)  NEUTRALIZATION