Question

For $ PbO+{{H}_{2}}\to Pb+{{H}_{2}}O $
Which of the following statements is wrong?
(A) $ {{H}_{2}} $ is the reducing agent.
(B) $ PbO $ is the oxidizing agent.
(C) $ PbO $ is oxidized to $ Pb $ .
(D) $ {{H}_{2}} $ is oxidized to $ {{H}_{2}}O $ .

Answer 1

Hint: We know that loss of electrons is known as oxidation and gain of electrons is known as reduction. If we say an element is an oxidizing agent then that means, it is undergoing reduction while it oxidizes another species and vice versa.

Complete answer:
 In redox reactions, the reactants undergo a change in their oxidation states. All the redox reactions involve two processes- a reduction process and an oxidation process. These two processes always occur simultaneously. Thus redox reactions are chemical reactions that involve the transfer of electrons between the reactants taking part in it.
When any substance is dissolved in water, it can have either an oxidizing property or a reducing property. However, it has been noted that, if we used ammonia as a solvent instead of water, then oxidizing agents either become weaker or show reducing characteristics. Diatomic iodine does not show strong oxidizing power in ammonia. It is also true that there is no acid which can exist in the solution which will be stronger than the conjugate acid of the solvent, in case of water it will be protonated water. This is called the leveling effect.
 $ \underset{+2}{\mathop{PbO}}\,+\underset{0}{\mathop{{{H}_{2}}}}\,\to \underset{0}{\mathop{Pb}}\,+\underset{+1}{\mathop{{{H}_{2}}O}}\, $ ; $ PbO $ is oxidized to $ Pb. $
Therefore, the correct answer is option C.

Note:
Remember that due to its properties peroxides are widely used as catalysts in chemical reactions. It is used along with Sodium Hydroxide to yield epoxide rings on carbonyl groups which have a double bond at the alpha position. It is also used as an initiator in free radical reactions due to its peroxide linkage.