Question

Can you please solve and provide the answer please

c. 10. Calculate the standard cell potential El using the given given data for the electrochemical cell constructed using the following reaction: Mn (s) + Ca**(aq) → Mnº(aq) + Ca(s). Half-reaction Standard reduction potential Mn* (aq) +2 e Mn(s) -1.185 V ca" (aq) +2 e Cd(s) -0.403 v a. +1.588 V d. +1.967 V b. +0.782 v e. -0.782 v -1.588 v 11. What is the value of the equilibrium constant for the oxidation of bromine by ozone at standard temperature.. 0,(8)+2H* (aq) +2e → H0(1) E° - +2.08 V Bro,"(g) +6 H(aq) +5e/Br, (s)+3H 0(1) E - +1.52 V 2.88 x 10° d. 3.47 x 10-10 b. 3.93 x 10 c. 6.47 x 1050 c. 94.6 12. Identify the correct half-reaction that applies to the oxidizing agent. (Note: The equation is not balanced. The reaction occurs in an acidic solution. 6,0, (aq) + C, H, OH(aq) → C,H,O(aq) + Crºs(aq) a. C,H,OH CH 0+2H* + +2 e b. 14H+Cr,0, +6e → 2Cr"* +7H,0 c. 14H*+Cr,0, 2Cr + 7H,0+80 d. C,H,OH+2 c +2H CHO+H,0 e. Cr,0, +3e" → Cr"* +7H,0 a.

Answer 1

Given reaction is Mn(s) + Cd⁺²(aq)  $\rightleftharpoons$ Mn⁺²(aq) + Cd(s)

Where the reduction half-reaction:

  Cd⁺²(aq) + 2e^-$\rightleftharpoons$  Cd(s) E^o_red = -0.403 V

the oxidation half-eaction is:

  Mn(s) $\rightleftharpoons$ Mn⁺²(aq) + 2e^-   E^o_red = -1.185 V

E^o of cell =  E^o_red of reduction half-raection -  E^o_red of oxidation half-reaction = -0.403 - (-1.185) = +0.782 V.

We should answer only one question.