Acetic acid + Ethanol <=> Ethylacetate + water Equilibrium occurs when
Concentrations are at a minimum but not equal
There is an equivalent amount of products to reactants
the reaction stops and K(forward) equals 1/K(reverse)
the rate forward equals the inverse of the reverse rate
There is no net change in concentrations
A)
this statement is false
concentrations may or may not be equal
B)
this is also false
because
products to reactants are not equivalent
C)
this statement is false
because the reaction does not stop
D)
this statement is false
because
we know that
equilibrium occurs when
rate of forward reaction is equal to rate of reverse reaction
E)
this statement is true
because
at equilibrium
the reaction still continues
only
there is no net change in concentrations
So
the answer is no net change in concentrations
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