Which of the following is an oxidation-reduction...

Which of the following is an oxidation-reduction reaction? A. Ba(NO$_3$)$_2$(aq) + K$_2$SO$_4$(aq) $\rightarrow$ BaSO$_4$(s) + 2 KNO$_3$(aq) B. Ag$^{+1}$(aq) + Cl$^{-1}$(aq) $\rightarrow$ AgCl(s) C. H$_2$SO$_3$(aq) + H$_2$O(l) $\rightleftharpoons$ HSO$_3^{-1}$(aq) + H$_3$O$^{+}$(aq) D. 3 H$_2$(g) + N$_2$(g) $\rightleftharpoons$ 2 NH$_3$(g)

Transcript

00:01 Hello students, in this video we are going to talk about redox reactions.

00:05 So, what are redox reactions? redox reactions are reactions in which both reduction and oxidation takes place.

00:14 Now, the common thing about reduction and oxidation is that there is a change in the oxidation state of the central atom.

00:24 So, now i'm going to give you some examples and we will see which one of them is a redox reaction and which one is not.

00:42 So, the first reaction is nai aqueous plus agno3 aqueous giving rise to agi solid plus nano3 aqueous.

01:00 Now, let us see the oxidation states.

01:03 So, here the oxidation state for na is plus 1 and for iodine it is minus 1, for ag it is plus 1, for no3 it is minus 1 and here also for ag it is plus 1 and i it is minus 1 and for na it is plus 1 and for no3 it is minus 1.

01:22 So, there is no change in oxidation.

01:27 So, this is not a redox reaction.

01:42 Now, let us take a look at another example.

01:48 For the second example, i have hcl aqueous reacting with lioh aqueous forming licl aqueous plus h2o liquid.

02:03 So, let us see the oxidation state.

02:06 Here h is plus 1, hcl is minus 1, here li is plus 1, oh is minus 1 and inside oh the o is minus 2 and h is plus 1.

02:19 Here also o is minus 2, h is plus 1 and cl is minus 1 and li is plus 1.

02:26 So, here also there is no change in the oxidation state.

02:34 So, it is not a redox reaction...

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