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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
Uses of Magnesium
- 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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