Silver bromide, AgBr, decomposes into silver (Ag) solid and bromine, (Br2) liquid at room temperature. Which ratio of silver to bromine is in the products of the reaction?(1 point)

Question

Responses

4:3
4:3

1:3
1:3

2:3
2:3

2:1
2:1

Answer 1

To determine the ratio of silver (Ag) to bromine (Br2) in the products of the decomposition of silver bromide (AgBr), we can start by looking at the balanced chemical equation for the reaction:

\[ 2 \text{AgBr} \rightarrow 2 \text{Ag} + \text{Br}_2 \]

From this equation, we can see that:

• For every 2 moles of AgBr that decompose, 2 moles of silver (Ag) are produced and 1 mole of bromine (Br2) is produced.

Therefore, the mole ratio of silver to bromine is:

• Silver (Ag) : Bromine (Br2) = 2 : 1

Thus, the correct response is 2:1.