Hydrogen and fluorine gas react to form hydrogen fluoride according to H2(g)+F2(
ID: 488816 • Letter: H
Question
Hydrogen and fluorine gas react to form hydrogen fluoride according to H2(g)+F2(g)2HF(g) H2 and F2 are mixed together and allowed to come to equilibrium. For the equilibrium mixture which of the following statements are correct (select ALL that apply)
The concentration of hydrogen gas remains constant
The concentration of hydrogen fluoride increases Reactions in both the forward and backwards directions are happening
The equilibrium constant is given by K equals fraction numerator left square bracket H subscript 2 right square bracket left square bracket F subscript 2 right square bracket over denominator left square bracket H F right square bracket end fraction
where [H2], [F2], and [HF] are the equilibrium concentrations
Explanation / Answer
for
H2(g)+F2(g)2HF(g)
The concentration of hydrogen gas remains constant --> False, it will be reacted/produced
The concentration of hydrogen fluoride increases --> false, it will increase since it is produced
Reactions in both the forward and backwards directions are happening --> True, even though rates are different, i.e. you will only see an overall rate to forward reaction
The equilibrium constant is given by K equals fraction numerator left square bracket H subscript 2 right square bracket left square bracket F subscript 2 right square bracket over denominator left square bracket H F right square bracket end fraction
K = [H2][F2] / [HF]^2 --> this is FALSE since products must always go ON TOP and reactants on the BOTTOM
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