Question

For which of the following reactions will a decrease in pressure shift the equilibrium to the left?
a. 2A2 (g) + B2 (g) 2A2B (g)
b. 2AB (g) A2 (g)+ B2 (g)
c. 2A2F3 (g) 4A (g) + 3F2 (g)
d. 2B (s) + 2HA (aq) 2BA (aq) + H2 (g)
I said C. But I feel as if I am wrong...

Answer 1

@Kainui

Answer 2

without the little --> signs in between the reaction and products it is kind of hard to determine what is a reactant and what is a product.

Just off looking at the little spaces between products and reactants, yes your answer of "C" would be correct.

Answer 3

wait i may have read some of the reactiosn incorrectly

Answer 4

one sec

Answer 5

Ohhh yeah you might need the arrows...
2A2 (g) + B2 (g) ---> 2A2B (g)
2AB (g) ---> A2 (g)+ B2 (g)
2A2F3 (g) ---> 4A (g) + 3F2 (g)
2B (s) + 2HA (aq) --> 2BA (aq) + H2 (g)

Answer 6

Ok now that I can see it C would actually shift the reaction to the right and not the left.

Answer 7

Ill just go through them. B would not work as their are an equal amount of gas on both left and right side. D. would not work as their an equal amount of gas on both left and right so pressure has no effect. Only A. because there are more gaseous reactants then products. The decrease in pressure would result in a decrease in concentration of 2A2 and B2 therefore the reaction would shift to the left.

Answer 8

Dude u truly do rock, thank you so freakin much! I totally understand it when you put it like that.

Answer 9

Im glad it makes sense now!. Feel free to tag me if you have any other questions !!