White phosphorus has the molecular formula p4 and sulfur has the molecular formula s8. how many grams of white phosphorus contain the same number of molecules as 6.41 g of sulfur?

To solve this problem, we must first convert sulfur the mass of sulfur into number of moles. We know that molar masses of the elements are:

S = 32 g / mol

P = 31 g / mol

Therefore the molecular forms has molar masses of:

S8 = 8 (32 g / mol) = 256 g / mol

P4 = 4 (31 g / mol) = 124 g / mol

Therefore converting mass to moles for S8:

moles S8 = 6.41 g / (256 g / mol) = 0.025 mol S8

This amount should be equal to P4, hence the number of moles of P4 should also be:

moles P4 = 0.025 mol P4

Converting to mass:

mass P4 = 0.025 mol (124 g / mol)

mass P4 = 3.1 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.