How do you balance $N i + C_{4} H_{8} N_{2} O_{2} \to N i {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $Ni + C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2$ ?

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How do you balance $N i + C_{4} H_{8} N_{2} O_{2} \to N i {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $Ni + C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2$ ?

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Answer 1 · 2016-01-28T05:44:51

$N i + 2 C_{4} H_{8} N_{2} O_{2} \to N i {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $Ni + 2C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2$

Explanation:

$N i + C_{4} H_{8} N_{2} O_{2} \to N i {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $Ni + C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2$
as there are 1 molecule nickel, 4 molecules of carbon, 8 molecules of hydrogen, 2 molecules of nitrogen, and 2 molecules of oxygen in left hand side
but 1 molecule of nickel, 8 molecules of carbon, 16 molecules of hydrogen, 4 molecules of nitrogen, and 4 molecules of oxygen
so, by multiplying $C_{4} H_{8} N_{2} O_{2}$ $C_4H_8N_2O_2$ by $2$ $2$ the equation will be balanced.

Answer 2 · 2016-01-28T12:32:18

${Ni}_{(aq]}^{2 +} + 2 C_{4} H_{8} N_{2} O_{2(aq]} \to Ni {(C_{4} H_{7} N_{2} O_{2})}_{2(s]} ⏐ ⏐ ↓ + 2 H_{(aq]}^{+}$ $"Ni"_text((aq])^(2+) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"H"_text((aq])^(+)$

Explanation:

The starting chemical equation given to you is actually incorrect.

This reaction takes place in aqueous solution and it involves the nickel(II) cation, ${Ni}^{2 +}$ $"Ni"^(2+)$ , not nickel metal, $Ni$ $"Ni"$ .

Reacting nickel(II) cations with dimethylglyoxime, $C_{4} H_{8} N_{2} O_{2}$ $"C"_4"H"_8"N"_2"O"_2$ , will produce an insolube solid called nickel dimethylglyoxime, $Ni {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $"Ni"("C"_4"H"_8"N"_2"O"_2)_2$ , which will precipitate out of solution.

The nickel(II) cations can be delivered to the solution by a soluble salt like nickel(II) nitrate, $Ni {({NO}_{3})}_{2}$ $"Ni"("NO"_3)_2$ .

The actual balanced chemical equation for this reaction can be written like this

${Ni}_{(aq]}^{2 +} + 2 C_{4} H_{8} N_{2} O_{2(aq]} \to Ni {(C_{4} H_{7} N_{2} O_{2})}_{2(s]} ⏐ ⏐ ↓ + 2 H_{(aq]}^{+}$ $"Ni"_text((aq])^(2+) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"H"_text((aq])^(+)$

The reaction involves two dimethylglyoxime molecules acting as chelating agents to form the nickel dymethylglyoxime complex.

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When the nickel(II) cations are delivered via nickel(II) nitrate, the reaction will produce

$Ni {({NO}_{3})}_{2(aq]} + 2 C_{4} H_{8} N_{2} O_{2(aq]} \to Ni {(C_{4} H_{7} N_{2} O_{2})}_{2(s]} ⏐ ⏐ ↓ + 2 {HNO}_{3(aq]}$ $"Ni"("NO"_3)_text(2(aq]) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"HNO"_text(3(aq])$

The nitrate anions, ${NO}_{3}^{-}$ $"NO"_3^(-)$ , are spectator ions in the reaction, meaning that they can be found on both sides of the chemical equation.

This reaction is used as a confirmation test for the presence of nickel(II) cations. Nickel dymethylglyoxime is a red precipitate.

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How do you balance $N i + C_{4} H_{8} N_{2} O_{2} \to N i {(C_{4} H_{8} N_{2} O_{2})}_{2}$ $Ni + C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2$ ?

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