A molecule that can h-bond will not always necessarily and does not have guarantee to have a higher boiling point than one than cannot have h-bond.
we can take an example of Pentan-2-one that cannot h-bond but instead of this it has a high boiling point that is 102.3 °C, while propan-1-ol can h-bond but it has a boiling point of 97.2°C, that is lower than the boiling point of Pentan-2-one.
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I can’t really explain in words so I took a pic of the work I did (Ignore the worksheet and just look at what I wrote to balance the equation.)
Photosynthesis is where carbon dioxide and water through light energy is converted in glucose and other organic compounds.
CCl4
(1x12.011 g/mol)+(4x35.45 g/mol) = 153.811 g
Answer:
What is the difference between real and ideal gas?
As the particle size of an ideal gas is extremely small and the mass is almost zero and no volume Ideal gas is also considered as a point mass. ... The molecules of real gas occupy space though they are small particles and also have volume.
An ideal gas is one that follows the gas laws at all conditions of temperature and pressure. To do so, the gas would need to completely abide by the kinetic-molecular theory. A real gas is a gas that does not behave according to the assumptions of the kinetic-molecular theory.
An ideal gas is defined as a gas that obeys gas laws at all conditions of pressure and temperature while A real gas is defined as a gas that does not obey gas laws at all standard pressure and temperature conditions.
