Balance each reaction, determine if they are ion-exchange, redox, or acid-base,

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)

Explanation / Answer

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.

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