This is the complete reaction. $(5$ Marks$)$

The reaction is not balanced. You should balance first.

$M{g}_3(P{O}_4{)}_2(aq)+Li(s)L{i}_{3}P{O}_4(aq)+Mg(s)$

Please write

a$.$ a$.$ The lonic reaction

b$.$ b$.$ Net lonic reaction

c$.$ C$.$ Reduced half$-$ reaction

d$.$ d$.$ Oxidized half$-$ reaction

e$.$ e$.$ Identify the oxidation and reduction reactant.

$2.$ Is the following reaction a redox reaction? Justify your answer by showing the oxidation numbers for each element and show your work. $(5$ Marks$)$

$2N{H}_{4}V{O}_3(aq)V_2{O}_5(s)+2N{H}_3(g)+H_{2}O(l)$

The following reactions are DISPROPORTIONATION reactions.

Please justify your answer by showing oxidation numbers for each elements and identify the reduced and oxidized elements.

$(5$ Marks$)$

DISPROPORTIONATION REACTION: A reaction in which some atoms of an element are oxidized and other atoms of the same element are reduced. $($Page $598$ Textbook$)$

a$.$ a$.Pb(s)+Pb{O}_2(s)+H_{2}S{O}_4(aq)2PbS{O}_4(s)+2H_{2}O(l)$

b$.3N{O}_2(g)+H_{2}O(l)2HN{O}_3(aq)+NO(g)$

For the following reactions:

Balance each equation using half$-$reactions in the given conditions, and find the reduced and Oxidized reactants.

a$.$ a$.Al+N{O}_3^{-}Al(OH{)}_4^{-}+N{H}_3$

$($ basic conditions$)$

a$.$ b$.Zn(s)+N{O}_3^{-}(aq)Z{n}^{+2}(aq)+N{H}_4^{+}(aq)$

$($ acidic conditions$)$

c$.Pb{O}_2(s)+I_2(s)P{b}^{2+}(aq)+I{O}_3^{-}(aq)($ acidic conditions$)$

d$.Mn{O}_4^{-}+Sn(OH{)}_4^{2-}Sn(OH{)}_6^{2-}+Mn{O}_2$

$($ basic conditions$)$

a$.$ e$.C{N}^{-}(aq)+Cr{O}_4$