# Oxidation Worksheet

Oxidation state is used to indicate the degeree of oxidation of an atom in chemical compound. Oxidation states are represented by integers, it can be any whole number which doesn’t have fractional part.

In simple words oxidation can be defined as, “The combination of a substance with oxygen.”

Questions:

1. A compound contains atoms X, Y and Z. The oxidation number of X is +3, of Y is +5 and of Z is -2. The possible formula of the compound is:

(a)    $XYZ_2$

(b)   $X_3(YZ_4)_3$

(c)    $Y_2(XZ_3)_3$

(d)   $X_3(Y_4Z)_2$

2. Which of the following represents a disproportionation reaction ?

(a)    $X_2 + 2OH^- \to XO^- + X^- + H_2O$

(b)   $2HCuCl_2 \overset{\text{Dilution}}{\underset{\text{with} H_2O} \rightarrow} Cu + Cu^{2+} + 4Cl^- + 2H^+$

(c)    $Cu_2O + H^+ \to Cu + Cu^{2+} + OH^-$

(d)   All of these

3. If M is the molecular weight of $FeC_2O_4$, then its equivalent weight in the conversion:

$FeC_2O_4 \to Fe^{3+} + CO_2$ is:

(a)    M/3

(b)   M/4

(c)    M/6

(d)   M/2

4. The ratio of coefficients of $HNO_3 ,Fe(NO_3 )_2 \text{and} NH_4NO_3$  in the following redox equation:

$Fe + HNO_3 \to Fe(NO_3)_2 + NH_4NO_3 + H_2O$

In the balanced form will be:

(a)    4 : 10 : 1

(b)   4 : 1 : 10

(c)    10 : 4 : 1

(d)   10 : 1 : 4

5. $(X) M n O^- _4 + (Y) H_2 o_2 \to 2Mn^{+2} + 5H_2O + 9O_2 + (Z) e^-$

In this reaction, values of (X), (Y) and (Z) are:

(a)    2, 5, 6

(b)   5, 2,6

(c)    3, 5, 6

(d)   2, 6, 6

6. The reaction in which hydrogen peroxide acts as a reducing agent is:

(a)    $2FeSO_4 + H_2SO_4 + H_2O_2 \to Fe_2(so_4)_3 + 2H_2O$

(b)   $2KI + H_2O_2 \to 2KOH + I_2$

(c)    $H_2SO_3 + H_2O_2 \to H_2SO_4 + H_2O$

(d)   $Ag_2O + H_2O_2 \to 2Ag + H_2O + O_2$

7. The oxidation number of phosporus in $Ba(H_2PO_2 )_2$ is:

(a)    +3

(b)   +2

(c)    -1

(d)   None of these

8. In the standardization of $Na_2S_2O_3$ using $K_2Cr_2O_7$ by iodometry, the equivalent weight weight of $K_2Cr_2O_7$ is

(a)    (molecular weight) / 2

(b)   (molecular weight) / 4

(c)    (molecular weight) / 3

(d)   Same as molecular weight

9. The reaction, $3Cl^-(aq) \to ClO_3(aq) + 2Cl^- (aq)$

Is an example of:

(a)    Reduction reaction

(b)   Oxidation reaction

(c)    Disproportionation reaction

(d)   Decomposition reaction

10. The pair of the compounds in which both the metals are in the highest possible oxidation state is:

(a)    $[Fe(CN_6)]^{3-}, [Co(CN)_6]^{3-}$

(b)   $CrO_2Cl_2, MnO^-_4$

(c)    $TiO_3, MnO_2$

(d)   $[Co(CN)_6]^{3-}, MnO_2$

11.  If the oxidation number of A is +2, of B is +5 and that of C is -2, the possible formula of the compound is:

(a)    $A_3(B_4)_2$

(b)   $A_3(BC_4)_2$

(c)    $ABC_3$

(d)   $A_3(BC_3)_2$

12. Oxidation number of iron in $Fe_{0.94}O$ is:

(a)    +2

(b)   94/200

(c)    2.13

(d)   +1

13. The oxidation state of oxygen in $O_2PtF_7$ is

(a)    0

(b)   +1/2

(c)    1

(d)   -1/2

14. A in the half reaction:

$A + OH^- \to O_2 + H_2O + 2e^-$ is:

(a)    $OH^-$

(b)   $OH_2$

(c)    $H_2O_2$

(d)   $HO^-_2$

15. In the conversion $NH_2OH \to N_2O$, equivalent weight of $NH_2OH$ is:

(a)    M/4

(b)   M/2

(c)    M/5

(d)   M/3

1.(b)     2. (d)     3. (a)     4. (c)     5. (a)

6. (d)    7. (d)     8. (c)      9. (c)     10. (b)

11. (b)      12. (b)     13. (b)     14. (d)     15. (b)

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