Question

Balance each reaction, determine if they are ion-exchange, redox, or acid-base, and determine the direction of the reaction and if they are reverisble or irreversible and explain why.

NH₄ NO(s) – N(g) + H₂(g)

N₂ (g) + O₂ (g) – NO (g)

N₂ (g) + H₂ (g) – NH₃ (g)

H₂O (g) - O₂ (g) + H₂ (g)

CaCO₃ (s) – CaO (s) + CO₂ (g)

Cl₂ (g) + H₂O (l) – HCl (aq) + HClO (aq)

NH₄ (s) – NH₃ (g) + HCl (g)

Fe (s) + H₂SO₄ (aq) – FeSO₄ (aq) + H₂ (g)

CO₂ (g) + H₂O (l) – H₂CO₃ (aq)

Mg (s) + H₂O (l) – Mg(OH)₂ (aq) + H₂ (g)

CH₃-COOH (aq) + H₂O (l) - CH₃-COO^- (aq) + H₃O⁺(aq)

Answer 1

Solution :-

Following are the answers for the each reaction equation.

1)unbalanced equation

NH4NO(s) --- > N2(g) + O2(g) + H2O(g)

Balanced equation is as follows.

2 NH₄NO₃(s) = 2 N₂(g) + O₂(g) + 4 H₂O(g)

This is redox reaction because the N is oxidized and O is reduced.

It is non reversible reaction because its decomposition reaction.

2)unbalanced equation.

N2(g) + O2(g) ---- > NO(g)

Balanced equation is as follows.

N2(g) + O2(g) ---- > 2NO(g)

Redox reaction because N is oxidized and O is reduced.

Can be reversible if NO is heated then reaction can be reversed.

3) unbalanced equation

N₂ (g) + H₂ (g) – NH₃ (g)

Balanced equation is as follows

N₂ (g) + 3H₂ (g) ----- >2 NH₃ (g)

Redox reaction

N is reduced and H is oxidized.

Can be reversible if NH3 is heated then it can reverse to produce H2 and N2

4) unbalanced equation

H₂O (g) ---- > O₂ (g) + H₂ (g)

Balanced equation is as follows

2H₂O (g) ---- > O₂ (g) + H₂ (g)

Redox reaction because O is oxidized and H is reduced.

Can be reversible.

5) CaCO₃ (s) ----- > CaO (s) + CO₂ (g) already balanced equation

Its decomposition reaction

Can be reversed if the CaO and CO2 are reacted then it will form CaCO3

6)unbalanced equation

Cl₂ (g) + H₂O (l) ----- > HCl (aq) + HClO (aq)

Already balanced equation

Its redox reaction because Cl is reduced and Cl is oxidized.

Not reversible.

7) unbalanced equation

NH₄ Cl(s) ----- > NH₃ (g) + HCl (g)

Balanced equation

2NH₄ Cl(s) ----- > NH₃ (g) +2 HCl (g)

Decomposition reaction

8) unbalanced equation

Fe (s) + H₂SO₄ (aq) ---- > FeSO₄ (aq) + H₂ (g)

Balanced equation

Fe (s) + H₂SO₄ (aq) ---- > FeSO₄ (aq) + H₂ (g)

Ion exchange reaction SO4^2- exchanged with Fe

Also redox reaction because Fe is oxidized and H is reduced.

Non reversible.

9)unbalanced equation

CO₂ (g) + H₂O (l) ----- >H₂CO₃ (aq)

Balanced equation

CO₂ (g) + H₂O (l) ----- >H₂CO₃ (aq)

ion exchange

it can be reversible because the H2CO3 is weak acid which is less stable so it reverse back to produce the CO2 and H2O

10) unbalanced equation

Mg (s) + H₂O (l) ----- > Mg(OH)₂ (aq) + H₂ (g)

Balanced equation

Mg (s) + 2H₂O (l) ----- > Mg(OH)₂ (aq) + H₂ (g)

Its redox reaction

Mg is oxidized and H is reduced

Non reversible

Because Mg can reduce the H

11)unbalanced equation

CH₃-COOH (aq) + H₂O (l) ----- >CH₃-COO^- (aq) + H₃O⁺(aq)

Balanced equation

CH₃-COOH (aq) + H₂O (l) ----- >CH₃-COO^- (aq) + H₃O⁺(aq)

Ion exchange reaction (acid base )

Reversible because the CH3COOH is weak acid.