Question

What happens chemically when quick lime is added to water-filled in the bucket?What happens chemically when quick lime is added to water-filled in the bucket?

Answer 1

Hint: Quick lime is a chemical compound in which the calcium and oxygen atoms are present, so its formula is CaO and also known as calcium oxide. When it is added to water either an exothermic reaction or endothermic reaction will take place.Quick lime is a chemical compound in which the calcium and oxygen atoms are present, so its formula is CaO and also known as calcium oxide. When it is added to water either an exothermic reaction or endothermic reaction will take place.

Complete step-by-step answer:
Quick lime is a chemical compound in which the calcium and oxygen atoms are present, so its formula is CaO and also known as calcium oxide. It is one of the industrially important compounds of calcium which is used for many purposes.
It is a white amorphous solid which is in powder form and its melting point is 2870 K.
When the quick lime or calcium oxide is treated with water, it forms slaked lime. Calcium oxide is an anhydrous form so, when it is treated with water, it forms hydrated quicklime (slaked lime). The formula of slaked lime is $Ca{{(OH)}_{2}}$. The reaction is given below:
$CaO+{{H}_{2}}O\to Ca{{(OH)}_{2}}$
But when the quick lime or calcium oxide is added to water, the reaction is vigorous and there is the evolution of heat because the reaction is an exothermic reaction. This process is known as slaking of lime and that is why it is named slaked lime. The evolution of a large amount of heat is due to the formation and breaking of a large number of lumps.Quick lime is a chemical compound in which the calcium and oxygen atoms are present, so its formula is CaO and also known as calcium oxide. It is one of the industrially important compounds of calcium which is used for many purposes.
It is a white amorphous solid which is in powder form and its melting point is 2870 K.
When the quick lime or calcium oxide is treated with water, it forms slaked lime. Calcium oxide is an anhydrous form so, when it is treated with water, it forms hydrated quicklime (slaked lime). The formula of slaked lime is $Ca{{(OH)}_{2}}$. The reaction is given below:
$CaO+{{H}_{2}}O\to Ca{{(OH)}_{2}}$
But when the quick lime or calcium oxide is added to water, the reaction is vigorous and there is the evolution of heat because the reaction is an exothermic reaction. This process is known as slaking of lime and that is why it is named slaked lime. The evolution of a large amount of heat is due to the formation and breaking of a large number of lumps.

Note: Industrially, the calcium oxide is formed when we heat the limestone in a rotator kiln at 1070-1270 K. The reaction is given below:
$CaC{{O}_{3}}\overset{1070-1270K}{\leftrightarrows}CaO+C{{O}_{2}}$
So, when the calcium oxide comes in contact with carbon dioxide, then it forms back to limestone. Industrially, the calcium oxide is formed when we heat the limestone in a rotator kiln at 1070-1270 K. The reaction is given below:
$CaC{{O}_{3}}\overset{1070-1270K}{\leftrightarrows}CaO+C{{O}_{2}}$
So, when the calcium oxide comes in contact with carbon dioxide, then it forms back to limestone.