Question

question 8 (1 point)
in the reaction: $\ce{kno_{3}(aq) + pbso_{4}(aq) \
ightarrow pb(no_{3})_{2}(aq) + k_{2}so_{4}(aq)}$, what is the reducing agent?
$\ce{kno_{3}(aq)}$
$\ce{pbso_{4}(aq)}$
$\ce{pb(no_{3})_{2}(aq)}$
$\ce{k_{2}so_{4}(aq)}$
there is no reducing agent

Explanation:

First, we need to check if this is a redox reaction. A redox reaction involves a transfer of electrons (change in oxidation states). Let's find the oxidation states of each element:

• In \(KNO_3\): \(K\) is \(+1\), \(N\) in \(NO_3^-\) is \(+5\), \(O\) is \(-2\).
• In \(PbSO_4\): \(Pb\) is \(+2\), \(S\) in \(SO_4^{2 -}\) is \(+6\), \(O\) is \(-2\).
• In \(Pb(NO_3)_2\): \(Pb\) is \(+2\), \(N\) in \(NO_3^-\) is \(+5\), \(O\) is \(-2\).
• In \(K_2SO_4\): \(K\) is \(+1\), \(S\) in \(SO_4^{2 -}\) is \(+6\), \(O\) is \(-2\).

Since there is no change in oxidation states for any element (all oxidation states remain the same), this is not a redox reaction. In a non - redox reaction, there is no reducing agent (a reducing agent is a substance that gets oxidized, i.e., its oxidation state increases, in a redox reaction).

Answer:

there is no reducing agent