232 - Considering the graphs below, which statement is incorrect? (The scales on the vertical axes of the graphs are equal.) [Figure: Two energy diagrams. Reaction I shows energy vs. reaction progress for $A(g) + D(g) \rightarrow 2AD(g)$ with activation energy $a$ and energy difference $l$. Reaction II shows energy vs. reaction progress for $2F(g) \rightarrow X(g) + Z(g)$ with energy levels $b$ and energy difference $l$.]
If energy $a$ kJ is supplied, both reactions I and II will proceed.
The mass of $E(g)$ released per mole consumed is $\dfrac{b}{2}$ kJ.
In reaction II, compared to reaction I, the products are more stable than the reactants.
The mass of energy released per mole of $AD(g)$ formed is greater than the energy released per mole of $X(g)$ formed.
\textbf{232 - Considering the graphs below, which statement is \underline{incorrect}?} (The scales on the vertical axes of the graphs are equal.)
\textit{[Figure: Two energy diagrams. Reaction I shows energy vs. reaction progress for $A(g) + D(g) \rightarrow 2AD(g)$ with activation energy $a$ and energy difference $l$. Reaction II shows energy vs. reaction progress for $2F(g) \rightarrow X(g) + Z(g)$ with energy levels $b$ and energy difference $l$.]}
\begin{enumerate}
\item If energy $a$ kJ is supplied, both reactions I and II will proceed.
\item The mass of $E(g)$ released per mole consumed is $\dfrac{b}{2}$ kJ.
\item In reaction II, compared to reaction I, the products are more stable than the reactants.
\item The mass of energy released per mole of $AD(g)$ formed is greater than the energy released per mole of $X(g)$ formed.
\end{enumerate}
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