How would applying an external pressure on the following equilibrium affects the distribution of iodide between the polar (aqueous) and non polar (varsol) phases?
I2+I^- --> I3^-
is the I2 gaseous, or solid? If gaseous, it shifts to the right.
all are aqueous
To understand how applying an external pressure would affect the distribution of iodide between the polar (aqueous) and nonpolar (varsol) phases, we need to consider Le Chatelier's principle. This principle states that when a system in equilibrium is disturbed by an external stress, the system will shift to counteract that stress and regain equilibrium.
In this case, the equilibrium reaction is:
I2 + I^- ⇌ I3^-
Let's consider the effects of applying an external pressure on the equilibrium:
1. Increasing the pressure:
When pressure is increased, the system will shift towards the side with fewer moles of gas to counteract the stress. In this reaction, there are no gas molecules involved, so increasing the pressure won't have any significant effects on the equilibrium distribution of iodide between the polar and nonpolar phases.
2. Decreasing the pressure:
Decreasing the pressure has the opposite effect. The system will shift towards the side with more moles of gas to counteract the decrease in pressure. Again, since there are no gas molecules involved in this reaction, decreasing the pressure won't have any significant effects.
Therefore, in the case of the given equilibrium reaction, applying an external pressure will not affect the distribution of iodide between the polar and nonpolar phases.