DATA TABLE DATA ANALYSIS 1. Calculate the calorimeter constant using the data you obtained in part I. Specific heat of w

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Data Table Data Analysis 1 Calculate The Calorimeter Constant Using The Data You Obtained In Part I Specific Heat Of W 1 (42.76 KiB) Viewed 37 times

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DATA TABLE DATA ANALYSIS 1. Calculate the calorimeter constant using the data you obtained in part I. Specific heat of water is 4.18 J/(g⋅∘C). This value should be small. If you get a large value or a negative value use 50 J/K for your calculations in part II and III. 2. For parts II and III, calculate the amount of heat energy, q, produced in each reaction. Use 1.03 g/mL for the density of all solutions. Use the specific heat of water, 4.18 J/(g⋅∘ C), for all solutions. Don't forget to use the calorimeter as part of your surroundings.
3. Calculate the enthalpy change, ΔH, for each reaction in terms of kJ/mol of each reactant. 4. Use the enthalpy change for reactions 5 and 6 above and Hess's law to determine the experimental molar enthalpy for Reaction 7. ΔHf​( experimental )= 5. How does the theoretical value compare to your experimental value? Calculate the % error.
In the space provided below, write the balanced reaction equations from the descriptions. Use the table of thermodynamic data in your text (or another approved resource) to calculate the molar enthalpy of the reactions ΔH( kJ/mol). Show your calculations. Reaction 1: The reaction of formation of gaseous ammonia, NH3​( g). 21​ N2​(9)+23​H2​(9)⟶2NH3​(9),ΔH1​ Reaction 2: Gaseous ammonia dissolves in water yielding aqueous ammonia, NH3​(aq). NH3​(9)+H2​O(1)⟶NH3​(−q) Reaction 3: The reaction of formation of gaseous hydrogen chloride, HCl(g). 1/2H2​(9)+21​Cl2​(9)⟶HCl(9) Reaction 4: Gaseous hydrogen chloride dissolves in water yielding aqueous hydrochloric acid. Hll(9)⟶HCl(aq) ​ Reaction 5: Aqueous solution of hydrochloric acid reacts with aqueous ammonia yielding aqueous ammonium chloride. NH3​ (aq) +HCl(aA) ​→NH4​Cl(a) ​S+H2​ Reaction 6: Solid ammonium chloride dissolves in water yielding aqueous ammonium chloride. NH4​Cl(s)→NH4​Cl(aq)​ In another piece of paper, arrange the six equations and their enthalpy values in such a way that when added algebraically they yield a seventh equation that describes the formation of a solid ammonium chloride. Shov the enthalpy value for reaction 7: