Search
Ask a question
0

choose the correct option


In Haber’s process 0.240 mole of Nitrogen, 3.9 moles of hydrogen are taken which
lead to the formation of 7.8 moles product in a 3.00 litres of reaction vessel at
375oC. Considering that equilibrium constant at this temperature is 41.2 Calculate
the value of reaction quotient (Q) and predict whether the reaction is in
equilibrium or it will proceed in either direction.
a) Q = 38.62 and reaction will be in equilibrium.
b) Q = 19.31 and reaction will proceed in forward direction.
c) Q = 38.62 and reaction will proceed in forward direction.
d) Q = 19.31 and reaction will proceed in backward direction.

Comments

The wording of this problem makes it seem as if the initial amount of nitrogen is 0.240 moles and the initial amount of hydrogen is 3.9 moles.  There is no way these could combine to make 7.8 moles of ammonia.  Are the three mole values given the amounts present at some point during the reaction?

1 Answer by Expert Tutors

Tutors, sign in to answer this question.
Rene M. | Rene taught AP Biology, AP Chemistry and AP Physics Rene taught AP Biology, AP Chemistry and...
5.0 5.0 (1 lesson ratings) (1)
0
When I crunched the numbers, I calculated a Q-value of 38.5 which is less than the K value of 41 that is given, thus the reaction will proceed in the forward direction.