Question

Cl2(g) + 2NaBr(aq) 2NaCl(aq) + Br2(l) The reaction given above is a single replacement reaction because: A. one of the reactants is a gas B. none of the reactants are solids C. chlorine replaces bromine D. the reaction proceeds spontaneously

Answer 1

Answer: C. chlorine replaces bromine

Explanation:

$Cl_2(g)+2NaBr(aq)\rightarrow 2NaCl(aq)+Br_2(l)$

A single replacement reaction is a chemical reaction in which more reactive element displaces the less reactive element from its salt solution.

This is a single replacement reaction in which chlorine replaces bromine from its aqueous solution. As chlorine is more reactive than bromine , it easily accepts electrons to convert to $Cl^{-}$ in $NaCl$ and $Br^-$ in $NaBr$ donates electrons to form $Br_2$.

The reactant chlorine is in gaseous state, $NaBr$ is in aqueous state. the product $NaCl$ is in aqueous state and bromine is in liquid state.

Answer 2

The answer is C. One item replacing another is a single replacement, but when two items trade places in two separate molecules it’s double replacement.