Home
Class 12
CHEMISTRY
To find the standard potential of M^(3+)...

To find the standard potential of `M^(3+)//M` electrode , the following cell is constituted : `Pt|M|M^(3+((.001moLL^(-1)|| Ag ^(+) ((0.01moLL^(-1))|` Ag. The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction `M^(3+)+ 3e^(-) to M` at 298 K will be :
(Given `E_(Ag^(+)//Ag^(@)` at 298 K = 0.80 Volt)

Text Solution

Verified by Experts

The correct Answer is:
0.3volt
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the emf of the following cell at 25^(@)C Ag(s)|AgNO_(3) (0.01 M)||AgNO_(3) (0.05 M)|Ag (s)

Calculate the emf of the following cell reaction at 298 K: Mg(s) +Cu^(2+) (0.0001 M) to Mg^(2+) (0.001M) +Cu(s) The standard potential (E^(Theta)) of the cell is 2.71 V.

The emf of the cell involving the following reaction, 2Ag^(+) +H_(2) rarr 2Ag +2H^(+) is 0.80 volt. The standard oxidation potential of silver electrode is:-

The e.m.f and the standard e.m.f of a cell in the following reaction is 5 V and 5.06 V at room temperature, Ni(s) + 2Ag^+(n) → Ni^(2+)(0.02M) + 2Ag(s) . What is the concentration of Ag+ ions?

Calculate the reduction potential for the following half cell reaction at 298 K. Ag^(+)(aq)+e^(-)toAg(s) "Given that" [Ag^(+)]=0.1 M and E^(@)=+0.80 V

The standard reduction potential of the Ag^(o+)|Ag electrode at 298K is 0.799V . Given that for AgI,K_(sp)=8.7xx10^(-17) , evaluate the potential of the Ag^(o+)|Ag electrode in a saturated solution of AgI . Also calculate the standard reduction potential of the I^(c-) |Agl|Ag electrode.

E_(M^(3+)//(M))^(@) = -0.036V , E_(M^(2+)//M)^(@)= -0.439V . The value of standard electrode potential for the change, M^(3+)(aq) + e^(-)rightarrow M^(2+) (aq) will be :

What is the cell entropy change ( in J K ^(-1)) of the following cell : Pt(s)|underset(p=1atm)(H_(2)(g))|CH_(2)underset(0.1M)(COOH,HCl)|underset(0.1M)(KCl(aq))|Hg_(2)Cl_(2)(s)|Hg The EMF of the cell is found to be 0.045 V at 298K and temperature coefficient if 3.4xxx10^(-4)V K^(-1) ( Given :K_(a(CH_(3)COOH))=10^(-5)M)

What is the cell entropy change ( in J K ^(-1)) of the following cell : Pt(s)|underset(p=1atm)(H_(2)(g))|CH_(2)underset(0.1M)(COOH,HCl)|underset(0.1M)(KCl(aq))|Hg_(2)Cl_(2)(s)|Hg The EMF of the cell is found to be 0.045 V at 298K and temperature coefficient if 3.4xxx10^(-4)V K^(-1) ( Given :K_(a(CH_(3)COOH))=10^(-5)M)