Home
Class 12
CHEMISTRY
The half -reactions of an electronchemic...

The half -reactions of an electronchemical cell are given below :
`MnO_4^(-)+8H^+(aq) +5e^(-)toMn^(2+)(aq)+4H_2O(l),E^o=+1.51V`
`Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^o=+0.15V`
Construct the redox equation from the standard from the standard potential of the cell and predict it the reaction is reactant favoured or product favoured.

Text Solution

Verified by Experts

At anode : `Sn_((aq))^(2+)rightarrow Sn_((aq))^(4+) + 2e^(-) ]xx5`
At cathode : `MnO_(4)^(-) (aq) + 8H_((aq))^(+) + 5e^(-)rightarrow Mn_((aq))^(2+) + 4H_(2)O_((1))]xx2`
Net cell reaction : `2MnO_(4) ^(-) + 5Sn_((aq))^(2+) + 16H_((aq))^(+)rightarrow2Mn_((aq))^(2+) + 5Sn_((aq))^(4+)+ 8H_(2)O_((1))`
`E_(cell)^(@) = E_(cathode)^(@) -E_(anode)^(@) = 1.51V - 0.15V - 0.15V = 1.36V`
Since, cell potential is positive therefore the reaction is product favoured.
Promotional Banner

Similar Questions

Explore conceptually related problems

Two half-reactions of an electrochemical cell are given below : MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-) toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51" V" Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-),E^(@)=-0.15" V"

Two half cell reactions of an electrochemical cell are given below : MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-),toMn^(2+)(aq)+4H_(2)O(l),E^(@)=+1.51V Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^(@)=+0.51V Construct the redox equation from the two half cell reactions and predict if the reaction favours formation of reactant or product shown in the equation.

Given that the standard electrode (E^(@)) of metals are : K^(+)//K=- 2.93 V, Ag^(+)//Ag = 0.80 V, Cu^(2+)//Cu = 0. 34 V, Mg^(2+)//Mg =- 2.37 V, Cr^(3+)// Cr =- 0.74 V, Fe^(2+)//Fe =- 0.44 V . Arrange these metals in an increasing order of their reducing power. Or Two half -reactions of an electrochemical cell are given below : MnO_4^(-) (aq) + 8 H^(+) (aq) + 5 e^(-) rarr Mn^(2+) (aq) + 4 H_(2) O (l) , E^(@) = + 1.51 V, Sn^(2+) (aq) to Sn^(4+) (aq) + 2e^(-) , E^(@) = + 0.15^(V) construct redox equation and predict if the reaction is reactant or product favoured.

Two half cell reactions of an electrons of an cell are given below : MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-) to Mn^(2+)(aq)+4H_(2)O(l) , E^(@)=+1.51 V Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^(@)=+0.15 V. Construct a redox equation from the two half cell reactions and predict if this reaction favours the formation of reactants or products as shown in the equation.

Given that standard electrode potentials (E^(@)) of metals are : K^(+)//K=-2.93" V",Ag^(+)//Ag=0.80" V",Cu^(2+)//Cu=0.34" V", Mg^(2+)//Mg=-2.37" V" Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-),E^(@)=-0.15" V" Construct the redox reaction equation from the two half-reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.

Complete the chemical equations : MnO_4^(-) (aq) + S_2O_3^(2-)(aq) + H_2O (l) to

Complete the chemical equations : MnO_4^(-) (aq) + H_2O_2(aq) + H^(+)(aq) to