Chemistry Experiment. Dr. Watson. Evaluating An Enthalpy Change That Cannot Be calculated Directly. Introduction. We were told that atomic number 11 hydrogen change decomposes on warming to give sodium carbonate, water and carbon dioxide as shown in the par below:- Â Â Â Â Â Â Â Â 2NaHCO3(s)--------> Na2CO3 (s) + pee (l) + CO2 (g) = DeltaH1 This was given as deltaH1 and we had to manoeuvre as fragmentise of the experiment. This however cannot be measured directly, only if can be found exploitation the enthalpy changes from 2 new(prenominal) reactions. These being that of sodium hydrogencarbonate and hydrochloric acidulent and also sodium carbonate and hydrochloric acid. We were given a call of instructions in how to imbibe on expose the experiment, which are given later. List of appliance Used. 1 x 500ml Beaker. 1 x Thermometer(-10 to 50oC). 1 x Polystyrene Cup. 1 x Weighing Balance. 1 x Weighing Bottle. 10 grams of atomic number 11 Hydrogencarbonate. 10 grams of Sodium Carbonate. A bottleful of 2 hero HCL. Diagram. Method. Three grams of sodium hydrogen carbonate was plodding out accurately using a weighting bottle and a balance. wherefore thirty centimetres cubed of 2 molar HCL was measured using a beat cylinder. The acid was and so placed into the polystyrene cup and its temperature was taken and enter using the thermometer.
The pre- weighted sodium hydrogencarbonate was and so added to the solution, and the final temperature was recorded. The contents of the cup were thusly emptied out and the cup was serve out with water and because exhaustively dried. This was do three measure for the sodium hydrogen carbonate so that I could pack any anomalies that were obtained. The experiment was then repeated in only the same behavior except sodium carbonate was used rather of sodium hydrogen carbonate. The results were then tabulated, this table is shown below. Results Table. Results Table... If you want to beget a full essay, sanctify it on our website:
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