Consider 55 mL of water (H2O) in a beaker and 55 mL of acetone [(CH3)2CO] in an identical beaker under identical conditions. Com
1 answer:
Answer:
More slowly than
Larger than
Weaker
Explanation:
The vapor pressure of a solution describes how quickly a solution will turn into vapour. If we say that a solution has a high vapour pressure, we are actually saying that the solution turns into vapour more quickly.
Acetone has a higher vapour pressure than water so acetone turns to vapour quicker than water.
Vapour pressure has a lot to do with the magnitude of intermolecular forces in solution. The stronger the magnitude of intermolecular forces, the lower the vapor pressure and the more slowly the solution evapourates.
So, the hydrogen bonds in water provides stronger intermolecular forces than dispersion and dipole interaction in acetone. Hence, water vaporizes more slowly than acetone.
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Answer: 7.98 grams of are produced if 10.7 grams of
are reacted.
Explanation:
To calculate the number of moles, we use the equation:
.....(1)
Putting values in equation 1, we get:
The chemical equation for the reaction is
By Stoichiometry of the reaction:
2 moles of produce = 1 mole of
So, 0.100 moles of produce=
of
Mass of =
Hence 7.98 grams of are produced if 10.7 grams of
are reacted.