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_(2)S_(2)O_(8)(aq)+2Kl(aq)to 2K_(2)SO_(4)(aq)+l_(2)(aq)

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

The cell in which the following reaction occurs: 2Fe^(3+)(aq)+2I^(-)(aq)rarr2Fe^(2+)(aq)+I_2(s) has E_(cell)^o=0.236 V at 298 K. Calculate the standard Gibbs energy and the equilibrium constant of the cell 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.

Write the half equations for each of the following redox reactions: (i) 2Fe^(3)+(aq)+2I(aq)rarrI_(2)(s)+2Fe^(2)+(aq) (ii) 2Na(s)+CI_(2)(g)rarr2NaCI(s) (iii)Mg(s)+CI_(g)rarrMgCI_(2)(s) (iv) Zn(s) + 2H^(+)(aq)rarrZn^(2)+(aq)+H_(2)(g) (V) 2k(s)+CI_(2)(g)rarr2kCI(s)

Write the anode and cathode reactions for the given cell reactions. S_(2)O_(8)^(2-)(aq)+2I^(-)(aq)rarr2SO_(4)^(2-)(aq)+I_(2)(s)

Identify the oxidant and reductant in the following reaction: 2K_4[Fe(CN)_6](aq) + H_2O_2(aq) rarr 2K_3[Fe(CN)_6](aq) + 2KOH (aq)

Write the half reaction for the following redox reaction. 2Fe^(3+)(aq) + 2l (aq) rarr I_2 (s) + 2Fe^(2+) (aq)