To determine whether the given chemical equation \( 8Ag_2S \rightarrow 10Ag + S_8 \) is balanced, we need to count the number of atoms of each element on both sides of the equation.
Reactants:
- Silver (Ag): \( 8 \times 2 = 16 \) atoms
- Sulfur (S): \( 8 \) atoms
Products:
- Silver (Ag): \( 10 \) atoms
- Sulfur (S): \( 8 \) atoms
Now we compare the number of atoms on both sides:
- Silver (Ag): 16 atoms (reactants) vs 10 atoms (products)
- Sulfur (S): 8 atoms (reactants) vs 8 atoms (products)
Based on this comparison, we can see that the number of silver atoms is not equal on both sides. Thus, the reaction is unbalanced.
Now let’s review the answer choices:
A. It is unbalanced because the products have fewer silver (Ag) atoms than the reactants. - This is true; there are fewer silver atoms in the products.
B. It is unbalanced because the number of sulfur (S) atoms in the products and reactants are the same. - This is misleading; while there is an equal number of sulfur atoms, the significant issue is the unbalance in silver atoms.
C. It is balanced because the mass of the reactants equals the mass of the products. - This is incorrect; the equation is not balanced.
D. It is balanced because the number of sulfur (S) atoms in the products matches the number in the reactants. - This is misleading; while the sulfur atoms are equal, the balance overall is not correct due to the silver atoms.
The best answer that explains the chemical reaction correctly is:
A. It is unbalanced because the products have fewer silver (Ag) atoms than the reactants.