Given the reaction at STP and at equilibrium: H2(g) + Cl2(g) → 2 HCl(9)
Which change will result in an increase in the
concentration of Cl2(g)?
A) decreasing the pressure of the system
B) decreasing the concentration of HCl(g)
C) increasing the concentration of H2(g)
D) increasing the concentration of HCl(9)

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)