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Fe2 + Lab Report

482 Words2 Pages

If there is a change in concentration, temperature, volume, or total pressure the equilibrium will change in order to react to the change. This concept was shwon throughout the experiment by the adding of new reagents and temperature changes. This was shown by the mixing of NH4NCS and Fe(NO3)3. The two chemicals together produced a dark red FeNCS2+. Since the solution became a dark red, the concentration of FeNCS2+ had increased. The darker solution means that the products are more favored at equilibrium which is called product favored and a lighter solution means that the reactants are more favored at equilibrium which is called reactant favored. When the group added more Fe(NO3)3 or NH4NCS to the second experiment, the system reacted by …show more content…

When tin chloride is added to the solution, Sn2+ took away positive charged ions; Fe3+ to Fe2+ (2Fe3+(aq) + Sn2+(aq) → 2Fe2+(aq) + Sn4+(aq)). This took away Fe3+ from the solution, causing the equilibrium to change to the reactants to balance the concentration of Fe2+. The solution turned a lighter color to increased rate of the reverse reaction. When AgNO3 was added to the solution, the silver nitrate broke down into Ag+ and …show more content…

The HPO4- ions messed up the equilibrium by removing Fe3+ ions from the solution (HPO42-(aq) + H2O(l) H2PO4-(aq) + OH-(aq), and Fe3+ (aq) + OH-(aq) = Fe(OH)3(s)). When the Fe3+ ion was taken away it caused the equilibrium to change to the reactants, so then it began to break apart the iron-thiocyanate complex ions. Adding NH3 into water changed to ammonium and hydroxide ions. The hydroxide ions reacted with the Fe3+ ions forming Fe(OH)3 (NH3·H2O(l) NH4+ (aq) + OH-(aq), and Fe3+ (aq) + OH-(aq) = Fe(OH)3(s)). This took away Fe3+ from the solution, causing the equilibrium to change to reactant favored. With the reactions that the group did in this experiment the equilibrium changes wherever in order to balance the ratio between the products and reactants. The system changes in favor of the side with the least amount of stuff. When the group added heat to the system resulted in a decrease in the concentration of FeNCS2+. When the increasing the temperature it the reverse reaction of the system was the take away the heat. In the ice bath, the opposite was observed. The system had an increase in the concentration of the product. So, when the ice bath was put in place the reaction was reactant

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