Question

write an equation for each of the following
i) displacement reaction
ii) precipitation reaction
iii) Redox reaction

Answer 1

Explanation:

Single Displacement Reactions

Single displacement reactions are reactions where one reactant replaces part of the other.

AB + C → AC + B

An example is the reaction between iron and copper sulfate to produce iron sulfate and copper:

Fe + CuSO4 → FeSO4 + Cu

Here, both iron and copper have the same valence. One metal cation takes the place of the other bonding to the sulfate anion.

Double Displacement Reactions

Double displacement reactions are reactions where the cations and anions in the reactants switch partners to form products.

AB + CD → AD + CB

An example is the reaction between silver nitrate and sodium chloride to form silver chloride and sodium nitrate:

AgNO3 + NaCl → AgCl + NaNO3

Precipitation reaction

All reactants and products that are soluble are written as ions, only the precipitate is written as if it were a molecule:

example: A+(aq) + B-(aq) + C+(aq) + D-(aq) → A+(aq) + D-(aq) + CB(s)

Redox reaction

the electrons. The equation should be balanced.

An example is given below of the reaction of iron(III) sulfate with magnesium.

Unbalanced reaction: Mg(s) + Fe2(SO4)3(aq) → Fe(s) + MgSO4(aq)

This reaction is split into two half-reactions, one that involves oxidation and one that involves reduction.

Reduction: Fe3+(aq) + 3e– → Fe(s)

Oxidation: Mg(s) → Mg2+(aq) + 2e–

This pair of half-reactions can be balanced by ensuring that both have the same number of electrons. To do this, multiply the oxidation half-reaction by 3 and the reduction half-reaction by 2, so that each half-reaction has 6e–.

2 Fe3+(aq) + 6e– → 2 Fe(s)

3 Mg(s) → 3 Mg2+(aq) + 6e–

Adding these two half reactions together gives the balanced equation:

2 Fe3+(aq) + 3 Mg(s) → 2 Fe(s) + 3 Mg2+(aq)

Notice that the sulfate ion (SO42-) is ignored. This is because it does not take part in the reaction; it is a spectator ion.

Complex Redox Reactions

For reactions in aqueous solution, these reactions can be more complex, and involve adding H+, OH−, and H2O in addition to electrons to compensate for oxidation changes.

Follow these steps when balancing acidic complex redox equations:

Write the oxidation and reduction half-reactions for the species including the element that is reduced or oxidized.

Balance both reactions for all elements except oxygen and hydrogen.

If the oxygen atoms are not balanced in either reaction, add water molecules to the side missing the oxygen. If the hydrogen atoms are not balanced, add hydrogen ions (H+).

Multiply the half-reactions by the appropriate number so that they have equal numbers of electrons.

Add the two equations to cancel out the electrons. The equation should be balanced.

Hope it helps..✌✌