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)?
1 answer
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.