1 gm of magnesium is burnt with 0.56gm of O2 in a closed vessel. Which reactant is left in excess and how much?

By BYJU'S Exam Prep

Updated on: September 25th, 2023

Magnesium is in excess and by 0.16.

(At. wt. Mg = 24 ; O₂ = 16)

The equation can be written as:

2Mg + O₂ → 2MgO

(s) (g) (s)

Therefore, in order to make 2 moles of MgO, 1 mole of O2 is needed.

Now we have to calculate the actual moles.

We know that

moles= mass/ molar mass

Mg= 1/24 = 0.041667

O₂ = 0.56/32 = 0.0175

Finding their ratio

Mole ratio of Mg: O₂ = 2:1

Now we have to find mass of Mg that reacts:

it implies that 2 moles of Mg and 1 mole of O2 react.

If 1 = 2

Then 0.0175 = 0.0175 x 2

= 0.035 moles of magnesium

mass of magnesium that reacts:

mass = moles x molar mass

Substituting the values we get

= 24 x 0.035

= 0.84 g

Accordingly, just 0.84 grams of the magnesium’s 1 gram reaction weight is utilised.

As a result, magnesium is overexposed and by 0.16

Table of content

Scientists use magnesium in medicine. It is commonly used to treat issues with the skin, attention deficit hyperactivity disorder (ADHD), anxiety, mania, post-operative recuperation, etc.
A great source of magnesium is the green leafy vegetable. Magnesium is also abundant in whole grains, seeds, and nuts, particularly almonds.
Magnesium is also present in the flashbulbs. Mg burns brightly, making it possible for photographers to shoot pictures in low light.

Summary:-

1 gm of Magnesium is burnt with 0.56gm of O2 in a closed vessel. Which reactant is left in excess and how much?

1 gm of magnesium is burnt with 0.56gm of O₂ in a closed vessel. Magnesium is in excess and by 0.16.

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