Refer to the periodic table given in your book and now answer the following questions:

(a) Select the possible non – metals that can show disproportionation reaction?

(b) Select three metals that show disproportionation reaction?

Asked by Pragya Singh | 1 year ago |  107

##### Solution :-

One of the reacting compounds must always contain an element that can exist in at least three oxidation states in disproportionation reactions.

(a) Because these elements can exist in three or more oxidation states, disproportionation reactions can occur.

(b) Because these elements can exist in three or more oxidation states, disproportionation reactions can occur.

Answered by Abhisek | 1 year ago

### Related Questions

#### Fluorine reacts with ice and results in the change:

Fluorine reacts with ice and results in the change:

$$H_{ 2 }O_{ (s) } \; + \; F_{ 2 \; (g) } \; \rightarrow \; HF_{ (g) } \; + \; HOF_{ (g) }$$

Justify that this reaction is a redox reaction

#### Depict the galvanic cell in which the reaction is

Depict the galvanic cell in which the reaction is:

$$Zn_{\left ( s \right )} \;+ \;2 \;Ag_{\left ( aq \right )}^{+} \;\rightarrow \;Zn^{2+}_{\left ( aq \right )} \;+ \;2 \;Ag_{\left ( s \right )}$$

Further show:

(i) which of the electrode is negatively charged?

(ii) the carriers of the current in the cell.

(iii) individual reaction at each electrode.

#### Given the standard electrode potentials,

Given the standard electrode potentials,

$$\dfrac{ K^{+}}{K}$$= –2.93V

$$\dfrac{ Ag^{+}}{Ag}$$ = 0.80V

$$\dfrac{Hg^{2+}}{Hg}$$ = 0.79V

$$\dfrac{ Mg^{2+}}{Mg}$$ = –2.37V

$$\dfrac{Cr^{3+}}{Cr}$$ = –0.74V

Arrange these metals in their increasing order of reducing power.

#### Arrange the given metals in the order in which they displace each other from the solution of their salts.

Arrange the given metals in the order in which they displace each other from the solution of their salts.

Al, Fe, Cu, Zn, Mg

#### An aqueous solution of AgNO3 with silver electrodes

Predict the products of electrolysis in each of the following:

(i) An aqueous solution of $$AgNO_{3}$$ with silver electrodes

(ii) An aqueous solution $$AgNO_{3}$$​ with platinum electrodes

(iii) A dilute solution of $$H_{2}SO_{4}$$​ with platinum electrodes

(iv) An aqueous solution of $$CuCl_{2}$$with platinum electrodes.