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Moving from Ethanol through Propanol to Butanol the physical properties like boiling points, surface tension and viscosity increases because of the increases in intermolecular interactions between the molecules of given compounds.
Explanation:
Ethanol, propanol and butanol all have hydroxyl groups in common, means all have hydrogen bond intractions between their molecules. So, taking the hydrogen bonding interaction constant we are left with only the difference in the number of carbon atoms.
Butanol has the greatest physical properties than other two because it has four carbon atom chain. So, as we know the London Dispersion forces or Van der Waal forces increases with increase in molecular size and chain length of hydrocarbon.
Therefore, the strength of London forces is greater in butanol than other two while ethanol has the smallest chain comparatively hence, lowest physical properties.
Answer:
PLZ HELP ME. This is my second time posting my question because the first time a person put a random answer. If you do not know the question please do not answer it and leave it to someone else. Thank you, and my question is on the attached image below.
Answer: Every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. ...
Use coefficients of products and reactants to balance the number of atoms of an element on both sides of a chemical equation.
Answer: I don’t know lol
Explanation: I am so sorry I thought this was easy
