Consider the following unbalanced equation:
Li2S(aq) + Bi(NO3)3(aq) → LiNO3(aq) + Bi2S3(s)
If 20.5 moles of Li2S(aq) reacts with an excess of Bi(NO3)3(aq), what is the theoretical yield of LiNO3(aq) in moles?

41 moles

Explanation:

The balanced equation for the reaction is given below:

3Li2S + 2Bi(NO3)3 —> 6LiNO3 + Bi2S3

The theoretical yield of LiNO3 can be obtained as follow:

From the balanced equation,

3 moles of Li2S produced 6 moles of LiNO3.

Therefore, 20.5 moles of Li2S will produce = (20.5 x 6)/3 = 41 moles of LiNO3

Therefore, the theoretical yield of LiNO3 is 41 moles

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

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