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
The balanced chemical equation for the decomposition of silver bromide is:
2 AgBr(s) → 2 Ag(s) + Br2(l)
From the balanced equation, you can see that for every 2 moles of AgBr, you obtain 2 moles of Ag and 1 mole of Br2.
Therefore, the ratio of silver to bromine in the products of the reaction is 2:1.
The balanced chemical equation for the decomposition of silver bromide (AgBr) can be written as:
2 AgBr (s) → 2 Ag (s) + Br2 (l)
From the equation, we can see that for every 2 moles of AgBr that decompose, we obtain 2 moles of Ag (silver) and 1 mole of Br2 (bromine). This means that the ratio of Ag to Br2 in the product of the reaction is 2:1.
To determine the ratio of silver to bromine in the products of the reaction, we need to use stoichiometry, which involves using balanced chemical equations.
The balanced chemical equation for the decomposition of silver bromide (AgBr) into silver (Ag) and bromine (Br2) can be written as:
2 AgBr(s) -> 2 Ag(s) + Br2(l)
According to the balanced equation, for every 2 moles of AgBr that decompose, we get 2 moles of Ag and 1 mole of Br2.
Therefore, the ratio of silver to bromine in the products is 2:1. This means that for every 2 moles of silver produced, 1 mole of bromine is also produced.
So, the ratio of silver to bromine in the product of the reaction is 2:1.