Assuming an efficiency of 49.50%, calculate the actual yield of magnesium nitrate formed from 130.7 g of magnesium and excess copper(ii) nitrate. mg+cu(no3)2⟶mg(no3)2+cu actual yield:

73.41 g

Explanation:

First find number of moles of Mg

n(Mg)

Second, find the number of moles of magnesium nitrate produced by this number of moles of magnesium.

The molar ratio is one is to one (using stoichiometric coefficients from the balanced equation). So 5.377 mol of magnesium produces 5.377 mol of magnesium nitrate

Third, find what mass of magnesium nitrate that is

mass(Mg(NO3)2) = mol * molar mass

                            = 5.377 mol * 148.3148 g/mol

                            = 148.3148 g

But the system is inefficient. It only has an efficiency of 49.50 so what will be the actual, not theoretical yield.

actual yield = efficiency * theoretical yield

                   =  49.5% * 148.3148 g

                    = 73.41  g

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.