Ultraviolet light is the correct answer
Hope this helps! If you dont understand balancing equations in general, say so in the comments, I’m happy to help
We know that:
Molar Mass H2O: 18 g/mol
<span>Molar Mass of Eugenol: 164 g/mol </span>
<span>Boiling point of H2O: 100 degrees C </span>
<span>Boiling point of Eugenol: 254 degrees C </span>
<span>Density of water: 1.0 g/mL </span>
<span>Density of Eugenol: 1.05 g/mL </span>
<span>Using formula:
V= [mole fraction x molar mass] / density </span>
<span>mH20: 0.9947 * 18
= 17.9046 / 1 g/mL
= 17.9046 </span>
<span>morg: 0.0053 * 164
= 0.8692/ 1.05 g/mL
= 0.8278 </span>
<span>V% = Vorg/(Vorg + VH2O) * 100 </span>
<span>(0.8278/18.7324) * 100 = 4.419% </span>
Yotal volume = 30 mL; therefore,
<span>0.0442 = (volume eugenol/30) </span>
<span>(m eug/mH2O) = (peug*164/pH2O*18) </span>
<span>(m eug/30) = (4*164/760*18) </span>
<span>m eug = about 1.44g and </span>
<span>
volume = mass/density
= 1.44/1.05
= about 1.37 mL </span>
Answer : Carbon tetrachloride, 
will show the greatest freezing point lowering.
Explanation :
For non-electrolyte solution, the formula used for lowering in freezing point is,
where,
= lowering in freezing point
= molal depression constant
m = molality
As per question, the molality is same for all the non-electrolyte solution. So, the lowering in freezing point is depend on the only.
That means the higher the value of , the higher will be the freezing point lowering.
From the given non-electrolyte solutions, the value of of carbon tetrachloride is higher than the other solutions.
Therefore, Carbon tetrachloride, will show the greatest freezing point lowering.
