The stoichiometry of the following reaction is `k_(2)S_(2)O_(8)(aq)+2Kl(aq)to 2K_(2)SO_(4)(aq)+l_(2)(aq)`

The stoichiometry of the following reaction is K_2S_2O_8(aq)+2kI(aq)rarr2K_2SO_4(aq)+I_2(aq)

The stoichiometry of the following reaction is K_2S_2O_8(aq)+2kI(aq)rarr2K_2SO_4(aq)+I_2(aq)

Balance the following equation : KCN (aq) +H_2SO_4(aq) rarr K_2SO_4(aq)+HCN(g)

Identify the oxidant and reductant in the following reactions 3K_(2)MnO_(4)(aq)+2H_(2)O(l)to2KMnO_(4)(Aq)+MnO_(2)(s)+4KOH(aq)

Why are the following reactions not redox reactions ? BaCl_(2)(aq)+H_(2)SO_(4)(aq)toBaSO_(4)(s)+2HCl(aq)

Observe the following reaction, 2NO_(2)(g) + 2OH^(-)(aq) to NO_(3)^(-)(aq) + H_(2)O (l) + NO_(2)^(-) (aq) in this reaction,

The experiment rate law for the reaction S_(2)O_(8)^(2-)(aq) + 2I^(ɵ)(aq) rarr 2SO_(4)^(2-) (aq) + I_(2)(aq) is k[S_(2)O_(8)^(2-)] [I^(ɵ)] . How would the rate change if (a) Concentration of S_(2)O_(8)^(2-) is halved. (b) Concentration of S_(2)O_(8)^(2-) and I^(ɵ) are halved.

The experiment rate law for the reaction S_(2)O_(8)^(2-)(aq) + 2I^(ɵ)(aq) rarr 2SO_(4)^(2-) (aq) + I_(2)(aq) is k[S_(2)O_(8)^(2-)] [I^(ɵ)] . How would the rate change if (a) Concentration of S_(2)O_(8)^(2-) is halved. (b) Concentration of S_(2)O_(8)^(2-) and I^(ɵ) are halved.

Complete the following reactions . (i) MnO_(4)^(-)(aq)+S_(2)O_(3)^(2-)(aq)+H_(2)O(l) to (ii) Cr_(2)O_(7)^(2-)(aq)+H_(2)S(g)+H^(+)(aq) to