Question

Write the balanced chemical equations for the following reactions.
a) Calcium hydroxide + Carbon dioxide $\to$Calcium Carbonate + Water.
b) Zinc + Silver nitrate $\to$Zinc nitrate + Silver.
c) Aluminum + Copper chloride $\to$Aluminum chloride + Copper.
d) Hydrogen + Chlorine $\to$Hydrogen chloride.
e) Ammonium nitrate $\to$Nitrogen + Carbon dioxide + Water.

Answer 1

Hint: The chemical equation should follow the law of conservation of mass. According to the law of conservation of mass, the number of dissimilar atoms of the elements in the reactants side should be equal to the number of elements in the product side.


Complete step by step answer:
- As per the question we have to write the balanced chemical equation for
a) Calcium hydroxide + Carbon dioxide $\to$Calcium Carbonate + Water.
$$Ca{(OH)}_2+C{O}_2\to CaC{O}_3+H_{2}O$$
In the above chemical reaction one mole of calcium hydroxide reacts with carbon dioxide and forms calcium carbonate and water as the products. Number of atoms on both sides of the chemical reaction is Ca–1, O−4, H−2, C−1.
b) Zinc + Silver nitrate $\to$Zinc nitrate + Silver.
$$Zn+2AgN{O}_3\to Zn{(N{O}_3)}_2+2Ag$$
In the above chemical reaction one mole of zinc reacts with 2 moles of silver nitrate and forms one mole of zinc nitrate and 2 moles of silver as the products. Number of atoms on both sides of the chemical reaction is Zn−1, Ag−1, N−1, O−3.
c) Aluminum + Copper chloride $\to$Aluminum chloride + Copper.
$$2Al+3CuC{l}_2\to 2AlC{l}_3+3Cu$$
In the above chemical reaction 2 moles of aluminum reacts with 3 moles of copper chloride and forms 2 moles of aluminum chloride and 3 moles of copper as the products. Number of atoms on both sides of the chemical reaction is Al−2, Cu−3, Cl−6.
d) Hydrogen + Chlorine $\to$Hydrogen chloride.
$$H_2+C{l}_2\to 2HCl$$
In the above chemical reaction one mole of hydrogen reacts with one mole of chlorine and forms 2 moles of hydrogen chloride as the products. Number of atoms on both sides of the chemical reaction is H−2, Cl−2.
e) Ammonium nitrate $\to$Nitrogen + Carbon dioxide + Water.
$$N{H}_{4}N{O}_3\to 2N_2+O_2+4H_{2}O$$
In the above chemical reaction one mole of ammonium nitrate decomposes and gives 2 moles of nitrogen, one mole of oxygen and 4 moles of water as the products. Number of atoms on both sides of the chemical reaction is N−4, H−8, O−6.


Note: If the number of atoms on both the sides of the chemical equation are not balanced then the chemical reaction is not called a balanced equation. As per law of conservation of mass the number of dissimilar atoms in a chemical reaction should be the same on both sides of the reaction.