Question

question 7 (1 point)
in the reaction: $ce{kno_{3}(aq) + pbso_{4}(aq) -> pb(no_{3})_{2}(aq) + k_{2}so_{4}(aq)}$, what is the oxidizing agent?
$ce{kno_{3}(aq)}$
$ce{pbso_{4}(aq)}$
$ce{pb(no_{3})_{2}(aq)}$
$ce{k_{2}so_{4}(aq)}$
there is no oxidizing agent

Explanation:

First, we need to determine the type of reaction. The given reaction is a double - displacement reaction (ions are exchanged between the reactants: $K^+$ from $KNO_3$ combines with $SO_4^{2 - }$ from $PbSO_4$, and $Pb^{2+}$ from $PbSO_4$ combines with $NO_3^-$ from $KNO_3$). In a double - displacement reaction, there is no change in the oxidation states of the elements. For a substance to be an oxidizing agent, it must cause another substance to be oxidized (which involves a change in oxidation state, usually the oxidizing agent is reduced, i.e., its oxidation state decreases). Since there is no change in oxidation states in this double - displacement reaction, there is no oxidizing agent.

Answer:

there is no oxidizing agent