0.378g grams of a compound is made up of 0.273g of Mg and 0.105g nitrogen. Find its empirical formula.

The empirical formula of the compound is .

Explanation:

Mass of magnesium in compound = 0.273 g

Mass of nitrogen in the compound = 0.105 g

Moles of magnesium =

Moles of nitrogen =

Form empirical formula divides the lowest value of moles of an element present with all the moles of elements present.

Magnesium

Nitrogen

The empirical formula of a compound:

The empirical formula of the compound is .

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.