I think the correct answer from the choices listed above is option B. It would be a leaf changing color in autumn <span>would a chemist be most likely to study. A chemist should be more interested in processes that chemical reactions are most likely to occur and changes in color can be one of the indications of such reactions.</span>
Answer:
C. Decrease the concentration of hydrogen gas
Explanation:
<u><em>Decreasing the concentration of hydrogen gas</em></u><em> would cause the equilibrium to shift to the right.</em>
According to Le Chatelier's principle, when a reaction is in equilibrium and one of the constraints affecting reactions is varied, the equilibrium will shift so as to annul the effects of the change.
Decreasing the concentration of dihydrogen sulfide will cause the equilibrium to shift to the left because as reactants are removed, more of the reactants would be formed.
Increasing the pressure of the system will also cause the equilibrium to shift to the left because the total number of moles of reactants is less than that of products. Hence, more of reactants would be formed with increased pressure.
Increasing the concentration of carbon disulfide will cause the equilibrium to shift to the left because as more of the products are added into the reaction, more of the reactants will begin to form.
<u>The only reason for the equilibrium to shift to the right causing more of the products to be formed is decreasing the concentration of hydrogen gas which happens to be one of the products. As more of the products are removed from the reaction, the equilibrium will shift to ensure that more products are formed.</u>
The correct option is C.
Answer:
A lone pair is a pair of electrons occupying an orbital in an atom or molecule and not directly involved in bonding.
Explanation:
It is true. Since it is very reactive with oxygen and water, it is kept in kerosene or some other some other oil
The given question is incomplete. The complete question is as follows.
A solution of chloroform (
) and acetone (
) exhibits a negative deviation from Raoult's law. This result implies that:
chloroform-chloroform interactions are stronger than chloroform-acetone interactions.
chloroform-chloroform interactions are weaker than chloroform-acetone interactions.
acetone-acetone interactions are stronger than chloroform-acetone interactions.
acetone-acetone interactions are weaker than chloroform-acetone interactions
chloroform-chloroform interactions are weaker than chloroform-acetone interactions AND acetone-acetone interactions are weaker than chloroform-acetone interactions.
Explanation:
It is known that when the forces between the particles of the mixture are stronger than the forces between the particles in the pure liquids then negative deviations from Raoult's law are observed.
Hence, when a solution of chloroform () and Acetone () will exhibit a negative deviation from Roult's law.
Then, chloroform-chloroform interactions should be weaker than chloroform-acetone interactions and acetone-acetone interactions must be weaker than Chloroform-Acetone interactions.
thus, we can conclude that for the given situation chloroform-chloroform interactions are weaker than chloroform-acetone interactions AND acetone-acetone interactions are weaker than chloroform-acetone interactions.
