Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2mg(s) + o2(g) → 2mgo(s) how many moles of o2 are consumed when 0.550 mol of magnesium burns?

0.275 moles of oxygen gas is consumed in the reaction.

Explanation:

We are given:

Moles of magnesium = 0.550 moles

For the given chemical reaction:

By Stoichiometry of the reaction:

2 moles of magnesium reacts with 1 mole of oxygen gas.

So, 0.550 moles of magnesium will react with = of oxygen gas.

Hence, 0.275 moles of oxygen gas is consumed in the reaction.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

they vary. it used to be meat, grain, bread, candy, beverages, donuts, and fruits/vegetables. now they added exercise in.