Question

How would you change the volume of the reaction container that holds the following reaction in order to increase the yield of SF6? S(s) + 3 F2(g) ↔ SF6(g)

1) Decrease the volume of the container. 2) Increase the volume of the container. 3) Do not change the volume of the container. 4) Cannot be predicted.\

How does an increase in temperature affect the equilibrium concentration of C and the equilibrium constant for the following reaction?
2 A(g) + B(g) ↔ 3 C(g) + D(g)           ΔH° = - 100 kJ

	[C] will increase and the equilibrium constant will increase.
	[C] will increase and the equilibrium constant will decrease.
	[C] will decrease and the equilibrium constant will increase.
	[C] will decrease and the equilibrium constant will decrease.

Answer 1

S(s) + 3 F2(g) ↔ SF6(g)

mol of GAS in products = 1

mol of GAS in reactats = 3

then, if we want to increase SF6, we need to favour products

we do this by increasing pressure, since pressurized systems favour the side with the LEAST moles

we can do this by decreasing th evolume

1) Decrease the volume of the container.

2)

this is exothermic, meaning it releases heat (as products form)

if we increase T, we favour the left side, which the reverse is endothermic

therefore

expect concnetation of C to drop

[C] will decrease and the equilibrium constant will decrease.

NOTE: the equilibrium CONSTANT, does not increases/decreases... they are probably talking about the reaction quotient Q, then