Predict the effect of removing chloride ions Now remove some of the free chloride ions by adding some silver nitrate (Hint: add 1 mL amounts of the silver nitrate successively until the equilibrium has been shifted instead ofa whole bunchat once): AgNOz(aq) <237 Ag+ NO3" Agt CI" AgCI(s) AgNO3(aq) CI- 0237 AgCI(s) NO3 Note by the above equation how Ag* scavenges free chloride ions by tying them up in a precipitate, and thus removes them from the solution 3. Predict the effect of adding HCI to the reaction Now do so in very small incremental steps until the equilibrium has shifted 4. Is the reaction as written endo or exothermic? Right click on the flask and choose thermal properties You can now change the temperature between 0 and 99 deg Heat or cool the system until you have perturbed the equilibrium Then apply LeChatlier's principal t0 determine if it iS exothermic or endothermic. 5. Allow the system t0 reach thermal equilibrium (constant temperature) Use the concentration values t0 determine K Now go to the thermal properties, change the temperature and click on the thermally isolated system option_ Determine the new K at the new temperature. From the new K at the new temperature determine if the System IS endothermic or exothermic:
