You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Representation of Cell

E⊝ values of ...

Question

$E^{⊝}$ values of some redox couples are given. On the basis of these values choose the correct option:
$E^{⊝}$ values:
$B r_{2} / B r^{-} = + 1.9; A g^{+} / A g (s) = + 0.8$
$C u^{2 +} / C u = + 0.34; I_{2} (s) / I^{-} = 0.54$ .

Cu will reduced

B r^{-}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Cu will reduce

A g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Cu will reduce

I^{-}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Cu will reduce

B r_{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A Cu will reduced $B r^{-}$
More positive the value of $E^{o}$ , greater is the tendency of the species to get reduced. On the basis of the given $E^{o}$ values, $B r_{2}$ is having highest $E^{o}$ value $(+ 1.90)$ , $C u$ will easily reduce $B r_{2}$ .

Suggest Corrections

Similar questions

$E^{⊖}$ values of some redox couples are given below. On the basis of these values choose the coorect option.
$E^{⊖}$ values :

$\frac{B r_{2}}{B r^{-}} = + 1.90 \frac{A g^{+}}{A g (s)} = + 0.80 \frac{C u^{2 +}}{C u (s)} = + 0.34 \frac{I_{2} (S)}{I^{-}} = + 0.54;$

(a) Cu will reduce $B r^{-}$
(b) Cu will reduce $A g$
(c) Cu will reduce $I^{-}$
(d) Cu will reduce $B r_{2}$

E^{0}

values of some redox couples are given below. On the basis of these values choose the correct option.

E^{0}

values

B r_{2} | B r^{-}

= +1.90V;

A g^{+} | A g_{(} s)

= +0.80V;

C u^{2 +} | C u_{(} s)

= + 0.34V;

I_{2 (s)} | I^{-}

= +0.54V

Q. The standard

E^{0}

values of few redox couples are

Z n^{2 +} / Z n = - 0.76 V

A g^{+} / A g = + 0.08 V

C u^{2 +} / C u = 0.34 V

. Choose the correct option?

The more positive the value of $E^{⊖}$ , the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.

E\ominus values :

$\frac{F e^{3 +}}{F e^{2 +}} = + 0.77 \frac{I_{2} (S)}{I^{-}} = + 0.54; \frac{C u^{2 +}}{C u} = + 0.34; \frac{A g^{+}}{A g} = 0.80 V$

(a) $F e^{3 +}$
(b) $I_{2} (s)$
(c) $C u^{2 +}$
(d) $A g^{+}$

The standard reducation potentials of

$Z n^{2 +} | Z n, C u^{2 +} | C u$ and $A g^{+} | A g$

are respectively -0.76, 0.34 and 0.8 V. The following cells were constructed.

a) $Z n | Z n^{2 +} | | C u^{2 +} | C u$

b) $Z n | Z n^{2 +} | | A g^{+} | A g$

c) $C u | C u^{2 +} | | A g^{+} | A g$

What is the correct order $E {^{0}}_{c e l l}$ of these cells?

Join BYJU'S Learning Program

E⊝ values of some redox couples are given. On the basis of these values choose the correct option:E⊝ values: Br2/Br−=+1.9; Ag+/Ag(s)=+0.8Cu2+/Cu=+0.34; I2(s)/I−=0.54.

The correct option is A Cu will reduced Br−More positive the value of Eo, greater is the tendency of the species to get reduced. On the basis of the given Eo values, Br2 is having highest Eo value (+1.90), Cu will easily reduce Br2.

$E^{⊝}$ values of some redox couples are given. On the basis of these values choose the correct option:
$E^{⊝}$ values:
$B r_{2} / B r^{-} = + 1.9; A g^{+} / A g (s) = + 0.8$
$C u^{2 +} / C u = + 0.34; I_{2} (s) / I^{-} = 0.54$ .

The correct option is A Cu will reduced $B r^{-}$
More positive the value of $E^{o}$ , greater is the tendency of the species to get reduced. On the basis of the given $E^{o}$ values, $B r_{2}$ is having highest $E^{o}$ value $(+ 1.90)$ , $C u$ will easily reduce $B r_{2}$ .