Which will have the lowest vapor pressure?
When comparing vapor pressures we need to be making comparisons at the same temperature. Thus at room temperature, the substance with the lowest boiling point will have the highest vapor pressure (easiest to get into the gas phase). The substance with the highest boiling point will have the lowest vapor pressure.
Why boiling point of NH3 H2O and HF is higher in their corresponding groups?
The higher boiling point of HF is thus due to stronger H-bonds. Explain why the boiling point of water (100 °C) is higher than both HF and NH3. The polarity of the O-H bonds in H2O is intermediate between that of H-F and N- H bonds.
Which has stronger intermolecular forces C25H52 or H2O?
Answer: C25H52 has stronger IM forces than H2O. (normal) melting and boiling points than H2O (50°C > 0°C, and 400°C > 100°C), it has the stronger IM forces between its molecules. are greater in C25H52.
What is the vapor pressure of HF?
The vapor pressure of HF has been redetermined between 273 and 303°K and is represented by log10P(torr) = 1·3428 − 947·26/T + 3·0233 log10T.
What compound has the highest vapor pressure at room temperature?
The HI has the highest vapor pressure at room temperature due to the following reasons. 1. These molecules do not have significant intermolecular…
Does HF or HBr have a higher vapor pressure?
HF will have a lower vapor pressure at -50oC than HBr.
How are the physical properties of H2O NH3 and HF affected by hydrogen bonding?
Explanation: Because of strong intermolecular hydrogen bonding, H2O, HF & NH3 exist as associated molecules. Therefore, their melting and Boiling point are much higher then those of the corresponding hydrides in their respective groups.
Why do water hydrogen fluoride and ammonia have unusually high boiling points?
Because ammonia (NH₃) and hydrogen fluoride (HF) both have high boiling points, they must have strong intermolecular forces. Each of these compounds contains an H atom directly bonded to one of the highly electronegative N, O, or F atoms, so their high boiling points result from their hydrogen bonding.
Why vapor pressure of CH4 is greater than that of NH3?
The intermolecular attractive forces occurring in, CH4 are only London dispersion forces. Hydrogen-bonding attractive forces are stronger forces compared to dispersion forces when atoms are in the second period. Therefore, NH3 has a higher boiling point compared to CH4.
What intermolecular forces are acting in the solid state of NH3?
London dispersion and hydrogen bonds.
What is the vapor pressure of water at 40 degrees Celsius?
55.3
Vapor Pressure of Water from 0 °C to 100 °C
| T °C | P (torr) |
|---|---|
| 40 | 55.3 |
| 41 | 58.3 |
| 42 | 61.5 |
| 43 | 64.8 |