Reaction mixtures of the following systems are prepared and allowed to come to equilibrium. Which (if any) of the systems will shift their equilibrium towards more products when the total pressure in the container is increased by decreasing the volume?
A) CO2(g) + H2(g) ⇔ H2O(l) + CO(g)
B) 2CO(g) + O2(g) ⇔ 2CO2(g)
C) 2NO(g) ⇔ N2(g) + O2(g)
D) N2O4(g) ⇔ 2NO2(g)
E) Ni(s) + 4CO(g) ⇔ Ni(CO)4(g)
F) 2C(s) + O2(g) ⇔ 2CO(g)
2007-04-20 20:21:49 · 3 answers · asked by bollocks 2 in Science & Mathematics ➔ Chemistry
a, b and e.
Lokk for those ones which have fewer moles of gas on the right.
2007-04-20 20:50:16 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
A i dont know what happens when one of the product is in liquid form
B forward diection
C backward directiom
D backward
E Forward
F Forward
2007-04-20 21:16:12 · answer #2 · answered by chem_fanatic 1 · 0⤊ 0⤋
when increasing the pressure:
a) shifts to the right
b) to the left
c) doesn't
d) to the left
e) to the right
f) to the left
2007-04-20 20:29:30 · answer #3 · answered by disillusion709 1 · 0⤊ 0⤋