Question

Is the following chemical equation balanced or unbalanced?

Balanced or Unbalanced

Answer 1

Unbalanced

Step-by-step explanation:

A balanced chemical equation must satisfy three conditions. It must:

1. Give the correct formulas for all reactants and products.
2. Have the same number of atoms of each element on both sides of the reaction arrow (balance mass).
3. Have the same net charge on each side of the reaction arrow (balance charge).

Your equation is unbalanced because it fails the first condition.

It satisfies the second condition, because there are 2 N atoms and 12 H atoms on each side of the arrow.

It also satisfies the third condition, because there are no charges on either side of the arrow.

However, a correctly balanced chemical equation must satisfy all three conditions.

Answer 2

This equation is balanced.

Step-by-step explanation:

To determine whether an equation is balanced or not, we must make sure that there are the same number of each type of atoms in both the reactants (on the left side of the equation) and the products (on the right side of the equation).

We can see that there are two atoms of nitrogen on the left side of the equation. When we look at the right side of the equation, we see that there are two molecules of NH6, with one atom of nitrogen each. Since 2 * 1 = 2, there are two atoms of nitrogen in the products as well. This means that the nitrogen atoms are balanced.

Next, we must look at the hydrogen atoms. There are 6 molecules of H2, which contains 2 atoms of hydrogen each. Since 6 * 2 = 12, there are 12 atoms of hydrogen in the reactants. On the right side of the equation, there are 2 molecules of NH6, which contains 6 atoms of hydrogen each. Since 2 * 6 = 12, there are 12 atoms of hydrogen in the products as well. Since there are 12 atoms on both sides of the equation, the hydrogen atoms are balanced.

Since both types of atoms that are presented in this equation are balanced, we can conclude that the overall equation is balanced.

Hope this helps!