Question

8Ag2S → 10Ag + S8
What is true about this chemical equation?
A. It is balanced because the products contain the same number of sulfur (S) atoms as the reactants.
B. It is unbalanced because the products contain fewer silver (Ag) atoms than the reactants.
C. It is balanced because the mass of the reactants is equal to the mass of the products.
D. It is unbalanced because the number of reactants is less than the number of products.

Answer 1

Answer:

Option (B) is correct

Explanation:

Because in reactants, there are 16 Silver(Ag) atoms but in product, there are onky 10 atoms of Silver(Ag).

Answer 2

B.It is unbalanced because the products contain fewer silver (Ag) atoms than the reactants.

Explanation:

$8Ag_2S\rightarrow 10Ag+S_8$

On Left hand side

Number of atoms of silver=$8\times 2$

Number of atoms of silver=16

Number of atoms of sulfur=8

On right hand side

Number of atoms of silver=10

Number of atoms of sulfur=8

Number of atoms of silver on LHS is not equal to number of atoms of silver on right side.

Number of atoms of silver in the product is less than the number of atoms of silver in the reactants.

Therefore, it is unbalanced reaction.

Hence, option B is true.

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