1. Each of the following reactions were in equilibrium when the pressure of their containers was doubled. Chose which way the reaction shifted after the pressure change:

Question

1. Each of the following reactions were in equilibrium when the pressure of their containers was doubled. Chose which way the reaction shifted after the pressure change:

Options are: Reactants, Products, Neither
i. 2NH3(g) <==> N2(g) + 3H2(g)
ii. 2Na3PO4(aq) + 3CaCl2(aq) <==> Ca3(PO4)2(s) + 6NaCl
iii. 2CO(g) + O2(g) <==> 2CO(s)
iv. 2HI(g) <==> H2(g) + I2(g)

what i got was
i. reactants
ii. products
iii. products
iv. neither but it got 0.75/1 so one of the answers were wrong. Could you tell which one was wrong (i-iv)?

Answer 1

ii is wrong. The effect of pressure and volume on liquids and solids is essentially zero and doubling the pressure will have no effect on the concentration of liquids or solutes.