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) 2C(s) + O2(g) ⇔ 2CO(g)
B) CO2(g) + H2(g) ⇔ H2O(l) + CO(g)
C) 2CO(g) + O2(g) ⇔ 2CO2(g)
D) 2NO(g) ⇔ N2(g) + O2(g)
E) N2O4(g) ⇔ 2NO2(g)
F) Ni(s) + 4CO(g) ⇔ Ni(CO)4(g)
2007-04-22 14:44:23 · 2 answers · asked by Mixed Asian 5 in Science & Mathematics ➔ Chemistry
The equilibrium will shift toward the side with the least amount of gas present.
A) reactants
B) products
C) products
D) reactants
E) reactants
F) products
2007-04-22 14:58:21 · answer #1 · answered by physandchemteach 7 · 0⤊ 0⤋
b,c,f
has less moles of gas on right side
2007-04-22 21:59:10 · answer #2 · answered by Professor Dopetastic Rockefeller 3 · 0⤊ 0⤋