Question

hClassify the following redox reactions:

(a) N2(g) + O2 (g) → 2NO(g)

(b) 2Pb(NO3)2


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Answer 1

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Classify the following redox reactions:

(a) N2(g) + O2 (g) → 2NO(g)

(b) 2Pb(NO3)2(s)

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$\Large\mathtt\green{ }\huge\underline\mathtt\red{Answer : }$

$N2(g) + O2 (g) → 2NO(g)N2(g)+O2(g)→2NO(g)$

(a) In this reaction, nitric oxide is formed by combination of the elemental substances, nitrogen and oxygen. So, it is an example of combination redox reaction.

$2Pb(NO3)2(s)2Pb(NO3)2(s)$

(b) It involves breaking down of lead nitrate into three components. So, it is an example of decomposition redox reactions.

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Answer 2

Answer:

Explanation:

Classify the following redox reactions:

(a) N2(g) + O2 (g) → 2NO(g)

(b) 2Pb(NO3)2(s)

In this reaction, the compound nitric oxide is formed by combination of elemental substances like nitrogen and oxygen. Since the oxidation number of nitrogen increases from 0 to +2 and of oxygen decreases from 0 to -2 therefore, it is a combination redox reaction.

(b)

In this reaction, lead nitrate decomposes to form three products, viz, lead oxide, nitrogen dioxide and oxygen. Since the oxidation number of nitrogen decrease from +5 in lead nitrate to +4 in NO2 in O2, therefore, it is a decomposition redox reaction.

(c)

In this reaction, hydrogen of water has been displaced by hydride ion to form dihydrogen gas. Therefore, it is a displacement reaction. Since in this reaction, the oxidation number of hydrogen increases from -1 in hydride ion to zero in dihydrogen gas and that of hydrogen decreases from +1 in water to zero in dihydrogen, therefore, it is a displacement redox reaction.

(d)

This is a disproportionation reaction since here the oxidation state of nitrogen decreases from +4 in NO2 to +3 in NO2– ion, as well as increases from +4 in NO2 to +5 in NO3 ion.