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Evaporation Rate of Various Compounds

The data below shows the change in temperature when four compounds are exposed to room temperature air over 2 minutes.

\begin{tabular}{|c|c|c|}
\hline Compound & \begin{tabular}{c}
Temperature \\
Change [tex]$\left({ }^{\circ} C \right)$[/tex]
\end{tabular} & Type of IMF \\
\hline A & -12.5 & DF \\
\hline B & -9.2 & DF \\
\hline C & -7.6 & [tex]$DF, DD$[/tex] \\
\hline D & -4.8 & [tex]$DF, DD, HB$[/tex] \\
\hline \multicolumn{3}{|c|}{ DF - dispersion forces, DD - dipole-dipole, HB - hydrogen bonding } \\
\hline
\end{tabular}

Which compound has the strongest intermolecular forces?

A. Compound D
B. Compound B
C. Compound A
D. Compound C

Sagot :

GinnyAnswer
To determine which compound has the strongest intermolecular forces (IMF) based on the change in temperature over 2 minutes, we should understand the relationship between temperature change and IMF strength. Generally, a compound that has a smaller change in temperature (less negative value) indicates stronger intermolecular forces because stronger IMFs will resist evaporation, leading to a smaller drop in temperature.

Let's examine the data:

1. Compound A: Temperature Change = -12.5°C
2. Compound B: Temperature Change = -9.2°C
3. Compound C: Temperature Change = -7.6°C
4. Compound D: Temperature Change = -4.8°C

Since we are looking for the compound with the strongest IMF, we need to identify which compound has the highest temperature change (the least negative number).

Here are the temperature changes ranked from the smallest change (strongest IMF) to the largest change (weakest IMF):

- Compound D: -4.8°C (least negative; strongest IMF)
- Compound C: -7.6°C
- Compound B: -9.2°C
- Compound A: -12.5°C (most negative; weakest IMF)

From this comparison, Compound D has the smallest temperature change, indicating that it has the strongest intermolecular forces.

Therefore, the compound with the strongest intermolecular forces is Compound D.
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