Question

3% Trial 4 What is the concentration of the stock H.O, solution? How much heat should be released when 10.0 mL of H., decompose? Your answer must be in units of kJ Trial Trial 2 Trial 3 Mass of H.Ozused (9) 0.055g 0.0589 0.052g Moles of H.O.decomposed (mol) 0.0016 0.0017 0.0015 Final Temperature (T) (°C) 38.00 138.4°C 13.1°C Initial temperature (T) ("C) 22:2°C 22.30 22.3°C Change in temperature: AT= T.-T (°C) 15.800 16.1°C 15.8°C How much heat was evolved by the reaction based on your experimental data: q(heat)decamp (J) 0.057g 0.6017 138.200 al.goc 16.3°C | 3.63 kJ 3.90k5 3,43kJ 3.88kJ What is the enthalpy of reaction AH experimental based on your data: (kJ/mol) acheat)decomposition moles H2O, decomposed 2268.7565 2294,1263 2284.6781 2282.3565 What is the average enthalpy of AH (k/mol) 2282.97 kJ/mol 1-2424.82 Theoretically, the decomposition reaction produces -98.2 kJ of heat per mole of H,O, decomposed. Calculate the relative percent error between this theoretical value and your average experimental enthalpy AHaug Hess's Law Calculation: Calculate the AH for the synthesis of hydrogen peroxide from its elements (H of formation). O2(g) + H2 (9) ► H2O2 AH° = 187.80 kJ/mol (Wikipedia) Use you experimental data for the decomposition of hydrogen peroxide and AH of formation for the synthesis of liquid water. End of Experiment.

need the Hess law calculations please!!!

Thanks

Answer 1

Having the reaction:

O2 + H2 = H2O2

You have the calculation of the law of hess:

ΔH = ΔHf H2O2 - ΔHf O2 - ΔHf H2 = 187.8 - 0 - 0 = 187.8 kJ / mol

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