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) Responses 2:1 2:1 2:3 2:3 4:3 4:3 1:3

Answer 1

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

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

From the equation, we can see that 2 moles of AgBr decompose to produce 2 moles of Ag and 1 mole of Br2.

Thus, the ratio of silver (Ag) to bromine (Br2) produced is:

• Silver (Ag): 2 moles
• Bromine (Br2): 1 mole

So, the ratio of silver to bromine is:

\[ \text{Ratio} = \frac{\text{Ag}}{\text{Br}_2} = \frac{2}{1} \]

Therefore, the answer is 2:1.