Question

the products of the following reaction in the balanced equation should be: br₂ + ki → o i + kbr₂ o 2i + 2kbr o i₂ + kbr o i₂ + 2kbr o no reaction occurs

Explanation:

Step1: Analyze the reaction type

This is a single - displacement reaction. Bromine (\(Br_2\)) is more reactive than iodine (\(I\)). In a single - displacement reaction \(A + BC
ightarrow AC + B\), here \(A = Br_2\), \(B = I\), \(C=K\). The general form of the reaction is \(Br_2+KI
ightarrow KBr + I_2\).

Step2: Balance the chemical equation

For the reaction \(Br_2+KI
ightarrow KBr + I_2\), we use the method of balancing atoms.

• Bromine atoms: On the left - hand side, we have \(2\) \(Br\) atoms in \(Br_2\). On the right - hand side, \(Br\) is in \(KBr\). To balance \(Br\) atoms, we put a coefficient of \(2\) in front of \(KBr\), so the equation becomes \(Br_2+KI

ightarrow 2KBr + I_2\).

• Potassium atoms: After putting a coefficient of \(2\) in front of \(KBr\), we have \(2\) \(K\) atoms on the right - hand side. So we put a coefficient of \(2\) in front of \(KI\) on the left - hand side. The balanced equation is \(Br_2 + 2KI=2KBr+I_2\).

Answer:

\(I_2 + 2KBr\) (corresponding to the option \(I_2+2KBr\))