Calculate the amount of heat released when [tex]$27.0 g H _2 O$[/tex] is cooled from a liquid at 314 K to a solid at 263 K. The melting point of [tex]$H _2 O$[/tex] is 273 K. Using the chart below, complete the steps to calculate the overall heat released in the process. Type in your answers using 3 digits on the right.
[tex]\begin{tabular}{|l|l|l|l|}\hline $\Delta T ( K )$ & Phase Change & Constant & Formula \\\hline $314 \rightarrow 273$ & Cool liquid & $C_{\text {p, lquid }}=4.184 J / g \cdot K$ & $q _1= cm \Delta T$ \\\hline 273 & Freeze liquid & $\Delta H_{\text {fusion }}=6.01 kJ / mol$ & $q _2= n \Delta H _{\text {fus }}$ \\\hline $273 \rightarrow 263$ & Cool solid & $C_{ p , \text { soluc }}=2.093 J / g \cdot K$ & $q _3= cm \Delta T$ \\\hline $314 \rightarrow 263$ & Liq $\rightarrow$ Sol & & $q_{\text {rot }}=q_1+q_2+q_3$ \\\hline\end{tabular}[/tex]
[tex]\begin{array}{l}
q_1=\square kJ \
q_2=\square kJ \
q_3=\square kJ \
q_4=\square kJ\n\end{array}[/tex]
Answer (2)
Many alcohols like ethanol have low boiling points, lower than water. Because of this, the ethanol molecules can overcome their inter molecular bonds that hold them in that liquid state. Hope this helps :)
Ethanol evaporates faster than water primarily due to its lower boiling point and weaker intermolecular forces. Although both substances can engage in hydrogen bonding, the stronger hydrogen bonds in water make it less volatile. Therefore, ethanol molecules require less energy to escape into the vapor phase.
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