Home
Class 12
CHEMISTRY
Consider the following equations for a c...

Consider the following equations for a cell reaction
`A+BiffC+D, E^(@)=x"volt",K_(eq)=K_1`
`2A+2Biff2C+2D, E^(@)=y"volt",K_(eq)=K_2` then:

A

`x=y, K_(1) = K_(2)`

B

`x= 2y, K_(1)^(2) = K_(2)`

C

`x=y, K_(1)^(2) = K_(2)`

D

`x^(2) = y, K_(1)^(2) = K_(2)`

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Similar Questions

Explore conceptually related problems

Consider the following equations for a cell reaction {:(A+Biff C + D,E^(o)=x" volt, K"_(eq)="k"_(1)),(2A+2Biff2C+2D,E^(o)=y" volt, K"_(eq)="k"_(2)):} then which of these is the correct relation ?

Consider the following equations for a cell reaction, A + B rarr C + D , E^(@) = x "volt", Delta G= Delta G_(1) 2A + 2B rarr 2C + 2D, E^(@) = y "volt", DeltaG = DeltaG_(2) Then,

Consider the following equilibrium reactions at 25^oC , A(g)+3B(g)hArr2C(g),K_(eq)=x A(g)+D(g)hArr2E(g),K_(eq)=y B(g)+D(g)hArrF(g),K_(eq)=z then the value of equilibrium constant for the reaction 2C+4DhArr2E+3F , at 25^oC is

In the following equilibria I:A+2B hArr C, K_(eq)=K_(1) II: C+DhArr 3A, K_(eq)=K_(2) III, 6B+D hArr 2C, K_(eq)=K_(3) Hence,

Consider the reaction fo extraction of gold from its ore Au +2CN^(-) (aq)+(1)/(4)O_(2) (g)+(1)/(2)H_(2)O rarr Au(CN)_(2)^(-) +OH^(-) Use the following data to calculate DeltaG^(@) for the reaction K_(f) [Au(CN)_(2)^(-)] = X {:(O_(2)+2H_(2)O +4e^(-)rarr4OH^(-),:,E^(@) =+0.41 "volt"),(Au^(3+)+3e^(-)rarr Au,:,E^(@) = +1.5 "volt"),(Au^(3+)+2e^(-)rarr Au^(+),:,E^(@) =+1.4 "volt"):}

For what value of k will the following system of linear equations have infinite number of solution :- 2x + 3y = 2 , (k + 2)x + (2k + 1)y = 2(k - 1)

Conisder the following reactions: I. A+B underset(k_(-1))overset(k_(1))hArr C II. C + B overset(k_(2))rarr D Then k_(1)[A][B]-k_(-1)[C]-k_(2)[C][B] is equal to (a) (-d[A])/(dt) (b) (-d[B])/(dt) (c) (d[C])/(dt) (d) (d[D])/(dt)

For a reaction A (s) + B^(2+) rarr B(s) + A ^(2+) , at 25^(@) C E^(o) "" _(cell) = 0.2955 V. Hence, K_(eq) will be :

Select the reaction for which the equilibrium constant is written as [MX_3]^2=K_(eq)[MX_2]^2[X_2]

If the E_(cell)^(@) for a given reaction has a positive value, then which of the following gives the correct relationship for the values of DeltaG^(@) and K_(eq) :-