Magnesium will burn in air to form both mg3n2 and mgo. what mass of each product would be found if burning a 3.26 g sample of magnesium to completion produces a combined total of 5.09 g of the two products

The mass of MgO formed is 3.502 grams and mass of formed is 1.587 grams.

Explanation:

We are given:

Total mass of magnesium reacted = 3.26 g

Total mass of products formed = 5.09 g

To calculate number of moles of a substance, we use the equation:

     .....(1)

The chemical equation for the formation of magnesium oxide follows:

Let 'x' grams of magnesium is reacting to form magnesium oxide.

Molar mass of Magnesium = 24.3 g/mol

Putting values in equation 1, we get:

Number of moles of magnesium =

By Stoichiometry of the reaction:

2 moles of magnesium produces 2 moles of MgO

So, moles of magnesium will produce moles of MgO

Molar mass of MgO = 40.3 g/mol

Putting values in equation 1, we get:

Mass of MgO =

Mass of magnesium oxide = = X grams

The chemical equation for the formation of magnesium nitride follows:

Mass of magnesium reacting = (3.26 - x)

Molar mass of Magnesium = 24.3 g/mol

Putting values in equation 1, we get:

Number of moles of magnesium =

By Stoichiometry of the reaction:

3 moles of magnesium produces 1 moles of

So, moles of magnesium will produce moles of

Molar mass of = 101 g/mol

Putting values in equation 1, we get:

Mass of

Mass of magnesium nitride = = Y grams

Total mass of the products = 5.09 grams

Putting values of 'X' and 'Y' in above equation, we get:

Mass of MgO =

Mass of

Hence, the mass of MgO formed is 3.502 grams and mass of formed is 1.587 grams.

the answer for sodium is 0.186

the answer for rubidium is 0.251

i would say b

explanation:

but i think i would need more information than that