Home
Class 12
CHEMISTRY
Write the following redox reactions usin...

Write the following redox reactions using half equations:
a. `Zn(s)+PbCl_(2)(aq)rarrPb(s)+ZnCl_(2)(aq)`.
b. `2Fe^(3+)(aq)+2I^(ө)(aq)rarrI_(2)(aq)+2Fe^(2+)(aq)`
c. `2Na(s)+Cl_(2)(g)rarr2NaCl(s)`
d. `Mg(s)+Cl_(2)(g)rarrMgCl_(2)(s)`
e. `Zn(s)+2H^(o+)(aq)rarrZn^(2+)(aq)+H_(2)(g)` .

Text Solution

Verified by Experts

(i) `Zn(s) rarr Zn^(2+)+2e^(-) ("oxidation") , Pb^(2+)(aq)+2e^(-) rarrPb(s)("reduction")`
Zn is oxidised to `Zn^(2+), Pb^(2+) ("reduction") , Pb^(2+)` is the oxidiser and Zn is the reducer
(ii) `2Fe^(3+)+2e^(-) rarr 2Fe^(2+) ("reduction") , 2I^(-)rarrI_(2)+2e^(-)("oxidation")`
`Fe^(3+)` reduced to `Fe^(2+) I^(-)` is oxidiased to `I_(2) , I^(-)` is the reducer and `Fe^(3+)` is the oxidiser
(iii)`2Na rarr2Na^(+)+2e^(-)("oxidation") , CI_(2)+2e^(-)rarr2CI^(-)`(reduction)
Na is oxidised to `Na^(+) "and" CI_(2)` is reduced to `CI^(-) , CI_(2)+2e^(-) rarr 2CI^(-)` (reduction )
Mg is oxidised o `Zn^(2+)` while `H^(+)` is reduced to `H_(2)` , Zn is ht reducer and `H^(+)` is the oxidiser
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • REDOX REACTIONS

    PRADEEP|Exercise NCERT (QUESTIONS AND EXERCISES WITH ANSWERS)|10 Videos

  • REDOX REACTIONS

    PRADEEP|Exercise NCERT(EXERCISE)|30 Videos

  • REDOX REACTIONS

    PRADEEP|Exercise Fill In Th Blanks|10 Videos

  • POLYMERS

    PRADEEP|Exercise IMPORTANT Questions (For Board Examination)|27 Videos

  • SOLUTIONS

    PRADEEP|Exercise IMPORTANT QUESTIONS FOR BOARD EXAMINATION|31 Videos

Similar Questions

Explore conceptually related problems

Write the folllowing redox rections using half equations (i) Zn(s) + PbCI_(2)(aq) rarr Pb(s)+ZnCI_(2)(aq) (ii) 2Fe^(3+)(aq)+2I^(-)(aq)rarrI_(2)(s)+2 Fe^(2+)(aq) (iii) 2Na(s)+CI_(2)(g)rarr2 NacI(s) (iv) Mg(s)+CI_(2)(g)rarrMgCI_(2)(s) (v)Zn(s)+2H^(+)(aq) rarr Zn^(2+)(aq)+H_(2)(g) In each of the reactions gien above mention (a) Which reactant is oxidized ? to what ? (b) which reactant is hte oxidiser ? (c )which reactant is reduced ? To what ? (d) which reactant is hte reducer?

Write the following redox reactions using half cell rections (i) Zn(s)+FeCI_(2)(aq)rarrZnCI_(2)(aq)+Fe(s) (ii)Mg(s)+CI_(2)(g)rarrMgCI_(2)(s) (iii)Mg(s)+2H^(+)(aq)rarrMg^(2+)(aq)+H_(2)(g)

Write the half equations for each of the following redox reactions: (i) 2Fe^(3)+(aq)+2I(aq)rarrI_(2)(s)+2Fe^(2)+(aq) (ii) 2Na(s)+CI_(2)(g)rarr2NaCI(s) (iii)Mg(s)+CI_(g)rarrMgCI_(2)(s) (iv) Zn(s) + 2H^(+)(aq)rarrZn^(2)+(aq)+H_(2)(g) (V) 2k(s)+CI_(2)(g)rarr2kCI(s)

Identify the oxidant and the reductant in the following reactions: a. Zn(s)+(1)/(2)O_(2)(g)rarrZn(s) b. Zn(s)+2H^(o+)(aq)rarrZn^(2-)(aq)+H_(2)(g)

Write the half reaction for the following redox reaction (a) 2Fe^(3+)(aq)+2I^(-)(aq)rarr2Fe^(2+)(aq)+I_(2)(aq) (b) Zn(s)+2H^(+)(aq)rarrZn^(2+)(aq)+H_(2)(g) (iii) Al(s)+3Ag^(+)rarrAl^(+3)(aq)+3Ag(s)

Write Nernst equation for the following cell reaction : Zn(s) | Zn^(2+)(aq)|| Cu^(2+)(aq) | Cu(s)

Write balanced net ionic equations for the following reactions in basic solution: (a) H_(2)O_(2)(aq)+ClO_(4)^(Ө)(aq) rarr ClO_(2)^(Ө)(aq)+O_(2)(g) (b) ( c) Cu(OH)_(2)(s) + N_(2)H_(4)(aq) rarr Cu(s)+N_(2)(g) (d) MnO_(4)^(Ө) + IO_(3)^(Ө)(aq)rarr MnO_(2)(s) + IO_(4)^(Ө)(aq)

In the reaction : 2Al(s) + 6HCl(aq) rarr 2 Al^(3+)(aq) + 6 Cl^(-)(aq) + 3H_(2)(g)

Identify the oxidant and reduction in the following reactions. (a) Zn(s) +1/2 O_2(g)rarrZnO(s) (b) CH_4(g) + 4Cl_2(g) rarr "CCl"_4(g) + 4HCl(g) (c) I_2(aq) +2S_2O_3^(2-)(aq)rarr2I^(-) (aq)+S_4O_6^(2-)(aq) (d) Zn(s)+2H^(+)(aq) rarr Zn^(2+) +(aq) +H_2(g)

Balance the following rebox reactions by ion electron method: a. MnO_(4)^(Θ)(aq)+I^(Θ)(aq) rarr MnO_(2)(s)+I_(2)(s) (in basic medium) b. MnO_(4)^(Θ)(aq)+SO_(2)(g) rarr Mn^(2+)(aq)+HSO_(4)^(Θ)(aq) (in acidic solution) c. H_(2)O_(2)(aq)+Fe^(2+)(aq) rarr Fe^(3+)(aq)+H_(2)O(l) (in acidic solution) d. Cr_(2)O_(7)^(2-)+SO_(2)(g) rarr Cr^(3+)(aq)+SO_(4)^(2-)(aq) (in acidic solution)

Home
Profile