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$E^o_{Cl_2/Cl^-} = 1.36\,V,$ $E^o_{Cr^{3+}/Cr}= -0.74\,V,$
$E^o_{Cr_2/O_7^{2-}/Cr^{3+}}=1.33\,V,$ $E^o_{MnO^-_4/Mn^{2+}} = 1.51\,V$
Among the following, the strongest reducing agent is
Step$-1$ : ${\text{A + E }} \rightleftharpoons AE$ (fast)
Step$-2$ :${\text{AE + A }} \to {A_2} + E$ (slow)
Step$-3$ :${{\text{A}}_2}{\text{ + B }} \to {\text{D}}$ (fast)
what rate law best agrees with this mechanism
Statement $I$ : The higher oxidation states are more stable down the group among transition elements unlike p-block elements.
Statement $II$ : Copper can not liberate hydrogen from weak acids.
In the light of the above statements, choose the correct answer from the options given below :
${B^{3 + }}_{(aq.)} + 3{e^ - } \to B(s)$ ; $E = 0.6\ Volt$
Using above information find the ion which will be deposited first at cathode if solution containing $A_{(aq.)}^{2 + }$ & $B_{(aq.)}^{ 3+ }$ is electrolysed