Shift ReactionThe goal of my experiment is to find out what happens to the heat of the zinc and copper sulfate solution when one of the variables is changed. Key variables:§ amount of copper sulfate solution§ amount of zincI I will study what happens to the temperature of the zinc and copper sulfate solution as the amount of zinc increases. The equation to show this reaction is: Zn + CuSO4 ® ZnSO4 + Cu The enthalpy change for the reaction is:²H = -217 kJ mole ¹ This means that if 1 mole of solution is used of each substance, the heat released will be 217,000 Joules.Apparatus: § 1 test tube § 20 ml of copper sulfate solution for each experiment § Zinc § Rubber stopper § Thermometer Prediction: I think that as the amount of zinc increases, the temperature of the solution will also increase. I used the following formula to predict some results of this experiment. q = Qmc where q = increase in temperature, Q = quantity of heat, m = mass of solution (20 g) and c = the specific heat capacity of water which = 4.18 Jg ¹K ¹ 0.65g Zinc ® 217000 joules1g Zinc ® 217000 = 3338 joules65So for 1g of zinc: 3338 =39°c increase20x4.18I can now use this formula proportionally to predict the results of my investigation.For 0.3g of zinc:0.3 x 39 = 12° c rise For 0.5g of zinc: 0.5 x 39 = rise of 19.5°c For 0.7g of zinc: 0.7 x 39 = rise of 27.3°c For 0.9g of zinc: 0.9 x 39 = rise of 35.1°cI used this information to predict the results of the increase in temperature I expect to see as the amount of zinc increases. I also used this information to plan my experiment.