Evaluating An Enthalpy Change That Cannot Be Measured Directly. Essay

Evaluating An Enthalpy Change That Cannot Be Measured Directly.Dr. Watson.Introduction.We were told that sodium enthalpycarbonate decomposes on heating to give sodiumcarbonate, pee and carbon dioxide as shown in the equation below-2NaHCO3(s)-------- Na2CO3 (s) + H2O (l) + carbon dioxide (g) = DeltaH1This was given as deltaH1 and we had to calculate as part of the experiment.This however cannot be thrifty directly, but can be found using the enthalpychanges from two other reactions. These being that of sodium hydrogencarbonateand hydrochloric acid and also sodium carbonate and hydrochloric acid.We were given a list of instructions in how to stockpile out the experiment, whichare given later.List of Apparatus Used.1 x 500ml Beaker. 1 x Thermometer(-10 to 50oC). 1 x Polystyrene Cup. 1 x measure Balance. 1 x Weighing Bottle. 10 grams of atomic number 11 Hydrogencarbonate. 10grams of Sodium Carbonate. A bottle of 2 molar HCL.Diagram.Method.Three grams of sodium hydrogen carbonate wa s weighted out accurately using a exercising weight bottle and a balance. Then thirty centimetres cubed of 2 molar HCL wasmeasured using a measuring cylinder. The acid was then placed into thepolystyrene shape and its temperature was taken and recorded using the thermometer.The pre-weighted sodium hydrogencarbonate was then added to the solution, andthe final temperature was recorded.The limit of the cup were then emptied out and the cup was washed out withwate...