Question

Write a balanced reaction equation for oxidation of carbon with concentrated nitric acid.
A. $C+4HN{{O}_{3}}\to C{{O}_{2}}+4N{{O}_{2}}+2{{H}_{2}}O$
B. $C+HN{{O}_{3}}\to C{{O}_{2}}+N{{O}_{2}}+2{{H}_{2}}O$
C. $2C+4HN{{O}_{3}}\to 2C{{O}_{2}}+4N{{O}_{2}}+2{{H}_{2}}O$
D. $C+2HN{{O}_{3}}\to C{{O}_{2}}+4N{{O}_{2}}+2{{H}_{2}}O$

Answer 1

A balanced chemical equation is the one in which equal number of atoms for each element involved in the reaction are represented in the reactant and product side. So we can write a balanced chemical reaction equation for oxidation of carbon with concentrated nitric acid as it is always inconsistent with the law of conservation of matter.

Complete step by step answer:
Carbon is oxidised with concentrated nitric acid.
When atoms lose or gain electrons to yield ions, or combine with other atoms to form molecules, their symbols are modified or combined to generate chemical formulas that appropriately represent their species. But the quantities of species undergoing chemical change involve balancing the chemical equation.
A balanced chemical reaction equation is always consistent with the law of conservation of matter. If an element appears in more than one formula on a given side of an equation, the number of atoms represented in each must be computed and added together.
Carbon denoted by “C” is oxidised by nitric acid denoted by $''HN{{O}_{3}}''$to produce carbon dioxide, water and nitrogen dioxide. (reddish brown gas)
$C+HN{{O}_{3}}\to C{{O}_{2}}+{{H}_{2}}O+N{{O}_{2}}$
The chemical equation is not a balanced one. We can balance it by simply summing the number of atoms on either side of the arrows and comparing these sums to ensure they are equal.
So the balance equation is
$C+4HN{{O}_{3}}\to C{{O}_{2}}+2{{H}_{2}}O+4N{{O}_{2}}$
And this may be confirmed by simply summing the number of atoms on either side of the arrow and comparing these sums to ensure they are equal.

Thus option (A) is the correct option.

Note:
Students should note that sometimes it is convenient to use fraction instead of integers as an intermediate coefficient in the process of balancing a chemical equation. And when the balance is achieved, the equation’s coefficient may then be multiplied by a whole number without upsetting the atom balance.