Use the following equation to solve the problems below POONO.2 - 2NO. PER
1 How many moles of Paris produced it 5.0 moles of wis reacted with excess PNO?
2. How many grams of KNO, is produced from the reaction of 6.6 moles of I?
3. If you complete the experiment and find that you actually produce 512 grams of KNO
what is your percent yield?
4. If you do the experiment again and this time, obtain an actual yield of 600 grams of
KNO, what is your percent yield for this experiment?

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.

u i forgot the answer?

2b2t

explanation:

2b2t