Half-reaction at anode:Half-reaction at cathode:+Use the References to access important values if needed for this question.+Enter electrons as e.Use smallest possible integer coefficients.States are not required. If a box is not needed, leave it blank.Standard Reduction Potentials (Volts) at 25 °C1.080Br₂ (1) + 2 e¯ →→→ 2 Br¨ (aq)O₂(g) + 4 H3O+(aq) + 4 e¯A 0.117 M neutral aqueous LaBr3 solution is electrolyzed under 1 atm pressure using platinum electrodes.(a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials.2 H₂O(1) + 2 e¨ ·H₂(g) + 2 OH-(aq) -0.828La³+ (aq) + 3 e¯ →→→→La (s)-2.370+6 H₂O(1)+(b) What is the expected decomposition potential?1.229++++

Anode is the electrode where the oxidation take place. Reduction potential of all the species are given. So the species having least reduction potential get oxidised. Here the species having least reduction potential is for La. But there is no solid La to oxidised. So oxidation take place for H2 at anode Cathode is the electrode in which reduction is occur. The species having highest reduction potential get reduced. Here the highest for O2. So O2 get reduced at cathode.So, the expected decomposition potential , = Ecathode-Eanode = 1.229 V - (-0.828 V) =2.057 VExpected decomposition potential = 2.057 V