What is the value of the reaction quotient, Q, for the cell?
`Ni(s)|Ni(NO_(3))_(2) (0.190 M)|| Cl_(2) (g), (1.0atm) |KCl(0.40M)`

The value of the reaction quotient Q for the cell Zn(s)|Zn^(2+)(0.01M)||Ag^(+)(0.05M)|Ag(s) is

The value of the reaction quotient Q for the cell Zn(s)∣Zn^(2+)(0.01M)∣∣Ag^(+)(0.25M)∣Ag(s) is :

The value of reaction quotient Q for the cell Zn(s)|Zn^(2+)(0.01M)||Ag^(o+)(1.25M)|Ag(s) is

Write the cell reaction for each of the following cells. Ni(s)|Ni^(2+)(aq)||Cu^(2+)(aq)|Cu(s).

Calculate the standard electrode potential of Ni^(2+) /Ni electrode if emf of the cell Ni_((s)) |Ni^(2+) (0.01M)| |CU^(2)| Cu _((s))(0.1M) is 0.059 V. [Given : E_(Cu^(2+)//Cu)^(@) =+0.34V

Calculate the emf of the cell Fe(s)+2H^(+)(1M)toFe^(+2)(0.001M)+H_(2)//(g),1 atm) (Given : E_(Fe^(+2)//Fe)=-0.44V)

For the cell, Pt|Cl_2(g,0.4"bar")|Cl^(-)(aq,0.1M)"||"Cl^(-)(aq),0.01M)|Cl_2(g,0.2"bar")|pt

Write the cell reaction and calculate the e.m.f. of the following cell at 298 K : Sn(s) |Sn^(2+) (0.004M)||H^(+) (0.020M) |H_(2)(g) (1 bar )| Pt(s) (Given E_(Sn^(2+)//Sn)^(@) = -0.14V ).

Calculate the emf of the cell in which the following reaction takes place : Ni(s)+2Ag^(+)(0.002M) to Ni^(2+) (0.160M) +2Ag(s) Given that E_("cell")^(Theta)=1.05V

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)