Balancing of Redox Reactions

Which of the following reactions are balanced

(i) ${\mathrm{Cr}}_2{\mathrm{O}}_{7\left(\mathrm{aq}\right)}^{2-}+3{\mathrm{H}}_2{\mathrm{S}}_{\left(\mathrm{g}\right)} +8{\mathrm{H}}_{\left(\mathrm{aq}\right)}^{+}\to 2{\mathrm{Cr}}_{\left(\mathrm{aq}\right)}^{3+}+3{\mathrm{S}}_{\left(\mathrm{s}\right)}+7{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$

(ii)  $2{{\mathrm{Cu}}^{2+}}_{\left(\mathrm{aq}\right)}+4{\mathrm{I}}^{-}{\text{}}_{\left(\mathrm{aq}\right)}\to {\mathrm{Cu}}_2{\mathrm{I}}_2{}_{\text{(}\mathrm{s})}+{\mathrm{I}}_2{}_{\left(\mathrm{g}\right)}$

The values of $\mathrm{x}$ and $\mathrm{y}$ in the following redox reaction,
$\mathrm{x} {\mathrm{Cl}}_2+6 {\mathrm{OH}}^{-}\to {\mathrm{ClO}}_3^{-}+\mathrm{y} {\mathrm{Cl}}^{-}+3 {\mathrm{H}}_2\mathrm{O}$ are

Balance the following equations by ion electron method.

$\mathrm{Zn}+{{\mathrm{NO}}_3}^{-}\to {\mathrm{Zn}}^{2+}+\mathrm{NO}$

The number of moles of ferrous oxalate oxidized by one mole of ${\mathrm{KMnO}}_4$ in an acidic medium is

In the chemical change:
$a{\mathrm{N}}_2{\mathrm{H}}_4+b{\mathrm{BrO}}_3^{-}⟶a{\mathrm{N}}_2+b{\mathrm{Br}}^{-}+6{\mathrm{H}}_2\mathrm{O},$ answer the following question:

What are the values of $\mathrm{a}$ and $\mathrm{b}$ in the reaction respectively:

${\mathrm{aN}}_2{\mathrm{H}}_4+{{\mathrm{bBrO}}_3}^{-}\to 3{\mathrm{N}}_2+2{\mathrm{Br}}^{-}+6{\mathrm{H}}_2\mathrm{O}$

What will be the ratio of number of moles of cerric ammonium sulphate required per mole of ferrous ammonium sulphate to the number of moles of ${\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4$ required per mole of ferrous ammonium sulphate?(Cerric ammonium sulphate and potassium permanganate are used as oxidising agents in acidic medium for oxidation of ferrous ammonium sulphate to ferric sulpahte.)

In the reaction

$8\mathrm{Al}+3{\mathrm{Fe}}_3{\mathrm{O}}_4⟶4{\mathrm{Al}}_2{\mathrm{O}}_3+9\mathrm{Fe}$

The Mn³⁺ ion is unstable in solution and undergoes disproportionation to give Mn²⁺, MnO₂ and H⁺ ion. Write a balanced ionic equation for the reaction. and stoichiometric coefficients for ${\text{Mn}}_{}^{3+}\text{,}{\text{MnO}}_2$ and H⁺ may be

In the balanced chemical equation
$\mathrm{I}{\mathrm{O}}_3^{-}+\mathrm{a}{\mathrm{I}}^{-}+\mathrm{b}{\mathrm{H}}^{+}\to \mathrm{c}{\mathrm{H}}_2\mathrm{O}+\mathrm{d}{\mathrm{I}}_2$
a, b, c and d are respectively.

The ratio of coefficients of $\mathrm{H}\mathrm{N}{\mathrm{O}}_3,\mathrm{F}\mathrm{e}(\mathrm{N}{\mathrm{O}}_3{)}_2$ and $\mathrm{N}{\mathrm{H}}_4\mathrm{N}{\mathrm{O}}_3$ in the following redox equation.
$\mathrm{F}\mathrm{e}+\mathrm{H}\mathrm{N}{\mathrm{O}}_3\to \mathrm{F}\mathrm{e}(\mathrm{N}{\mathrm{O}}_3{)}_2+\mathrm{N}{\mathrm{H}}_4\mathrm{N}{\mathrm{O}}_3+{\mathrm{H}}_2\mathrm{O}$ in the balance form will be

The reaction Cl₂ (g) + $S_2{O}_3^{2-}\to S{O}_4^{2-}$ + Cl^– is to be carried out in basic medium. Starting with 0.15 mole of Cl₂ , 0.010 moles of $S_2{O}_3^{2-}$ and 0.30 moles of OH^– , how many milli moles of OH^– will be left in solution after the reaction is complete ? Assume no other reaction occurs.

When copper is treated with a certain concentration of nitric acid, nitric oxide and nitrogen dioxide are liberated in equal volumes according to the equation,
$\mathrm{xCu}+{\mathrm{yHNO}}_3\to \mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2+\mathrm{NO}+{\mathrm{NO}}_2+{\mathrm{H}}_2\mathrm{O}$
The coefficients of x and y are respectively

How many mole of ${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4$ oxidized separately by one mole of $\mathrm{K}\mathrm{M}\mathrm{n}{\mathrm{O}}_4$ in acid medium.

How many moles of $\mathrm{F}\mathrm{e}\mathrm{S}{\mathrm{O}}_4$ oxidized separately by one mole of $\mathrm{K}\mathrm{M}\mathrm{n}{\mathrm{O}}_4$ in acid medium?

The reaction

$5{\mathrm{H}}_2{\mathrm{O}}_2+\mathrm{X}\mathrm{C}\mathrm{l}{\mathrm{O}}_2+2\mathrm{O}{\mathrm{H}}^{-}\to \mathrm{X}\mathrm{C}{\mathrm{l}}^{-}+\mathrm{Y}{\mathrm{O}}_2+6{\mathrm{H}}_2\mathrm{O}$ is balanced if -

In the following reaction:

$\mathrm{x}\mathrm{ }\mathrm{K}\mathrm{M}\mathrm{n}{\mathrm{O}}_4+\mathrm{y}\mathrm{ }\mathrm{N}{\mathrm{H}}_3⟶\mathrm{K}\mathrm{N}{\mathrm{O}}_3+\mathrm{M}\mathrm{n}{\mathrm{O}}_2+\mathrm{K}\mathrm{O}\mathrm{H}+{\mathrm{H}}_2\mathrm{O}$

X and y are

In the following equation :
$\mathrm{C}\mathrm{l}{{\mathrm{O}}_3}^{–}+\mathrm{ }6{\mathrm{H}}^{+}+\mathrm{ }\mathrm{X}\to \mathrm{C}{\mathrm{l}}^{–}+3{\mathrm{H}}_2\mathrm{O}$, then $\mathrm{X}$ is -

In balancing the half reaction, ${\mathrm{S}}_2{\mathrm{O}}_3^{2-}\to \mathrm{S}\left(\mathrm{s}\right)$, the number of electrons that must be added is -