The boiling point of water, ethanol, toluene and butan-2-ol are 373.0k, 351.3k, 383.6k and 372.5k respectively. Which liquid has the highest vapour pressure at 323.0k?
water
toluene
ethanol
butan-2-ol
none
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From the New School Chemistry textbook,
"Condensation increases as Vapour Pressure rises, i.e. as more and more liquid particles evaporate."
So, for the VP to rise, they'd have to get to that "evaporation point" faster. Hence, the one with the smaller boiling point will reach that point faster. So, at 323K, ethanol having the smallest boiling point will most likely have the highest vapour pressure.
* Boiling Point: This is the temperature where a liquid turns into a gas.
* Vapor Pressure: Vapor pressure is like how much a liquid wants to become a gas. A liquid with a higher vapor pressure turns into a gas more easily.
* Relationship: Liquids with lower boiling points have higher vapor pressures at the same temperature.
Here's how we can figure it out:
* Look at the boiling points:
* Water: 373.0 K
* Ethanol: 351.3 K
* Toluene: 383.6 K
* Butan-2-ol: 372.5 K
* Find the lowest boiling point: Ethanol has the lowest boiling point (351.3 K).
* The answer: Because ethanol has the lowest boiling point, it will have the highest vapor pressure at 323.0 K.
So, the answer is C. ethanol.
The Answer is Ethanol.
The boiling point of a liquid is INVERSELY PROPORTIONAL to its Vapour pressure. I.e the liquid with the lowest boiling point will has the highest Vapour pressure, and that's Ethanol from that list.
Okay to understand this question properly
Y'all should go and read "COLLIGATIVE PROPERTIES"
Boiling point elevation, vapour pressure lowering, freezing point depression and so on
