Question

What is quicklime? And what occurs when a 10 g mass of this material reacts with the carbon dioxide liberated from the decomposition of 1.80 g of glucose?

Answer 1

Hint: Calcium oxide (CaO), often known as quicklime or burned lime, is a chemical substance that is frequently utilised. At room temperature, it is a white, caustic, alkaline, crystalline solid. The word "lime" refers to calcium-containing inorganic compounds that are mostly composed of carbonates, oxides, and hydroxides of calcium, silicon, magnesium, aluminium, and iron. Quicklime, on the other hand, refers to the single chemical molecule calcium oxide. Free lime is calcium oxide that has not been processed and has not reacted in construction materials such as cement.

Complete answer:
The mole is the International System of Units' basic unit of material quantity (SI). It is defined as a collection of precisely \[6.02214076\times {{10}^{2}}^{3}\] particles, which may be atoms, molecules, ions, or electrons.
The Avogadro number (\[6.02214076\times {{10}^{2}}^{3}\]) was set such that the mass of one mole of a chemical compound in gram is numerically equivalent to the average mass of one molecule of the compound in daltons for most practical applications.
$\text{Number of moles = }\dfrac{\text{Given mass}}{\text{Molecular mass}}$
And when we look at the $1: 1$ reaction taking place here
$\text{CaO}(s)+\text{C}{{\text{O}}_{2}}(g)\xrightarrow{\text{water}}\text{CaC}{{\text{O}}_{3}}(s)$
Moles of calcium oxide $\equiv \dfrac{5.6 \cdot g}{56.08 \cdot g \cdot m o l^{-1}}=0.10 \cdot m o l$
And according to the question glucose combusts according to following reaction ${{C}_{6}}{{H}_{12}}{{O}_{6}}(s)+6{{O}_{2}}(g)\to 6C{{O}_{2}}(g)+6{{H}_{2}}O(l)$
And hence the moles of carbon dioxide liberated can be given as $\dfrac{1.80 \cdot g}{180.16 \cdot g \cdot m o l^{-1}} \times 6 \equiv 0.600 \cdot m o l$
As a result of the EXCESS carbon dioxide, the reagent $C{{O}_{2}}$ is in excess.
And hence we get $0.10 \cdot$ mol $\mathrm{CaCO}_{3}$, which initiates a mass of$0.10 \cdot \mathrm{mol} \times 100.09 \cdot \mathrm{g} \cdot \mathrm{mol}^{-1}=10.0 \cdot g$ calcium carbonate.
0.600 moles of carbon dioxide is liberated.

Note:
The mole is simply a particle count. The particles being counted are usually chemically identical entities that are individually unique. A solution, for example, might include a specific number of dissolved molecules that are more or less independent of one another. The component particles of a solid, on the other hand, are stable and bonded in a lattice structure, yet they may be separated without losing their chemical identity. As a result, the solid is made up of a specific number of moles of these particles. In certain situations, such as diamond, when the entire crystal is basically a single molecule, the mole is nevertheless employed to indicate the number of atoms bonded together instead of a count of numerous molecules.