Question

THERM OCHEMISTRY I1: HESS'S LAW OF CONSTANT HEAT SUMMATION ADVANCED PROBLEM ASSIGNMENT Dare Section Name READ THE EXPERIMENTAL DISCUSSION FIRST SHOW CALCULATION SET-UPI SIGNS! SIGNIFICANT FIGUREESi The 1.00 M solutions of HNO, and NaOH used in this experiment are prepared by diluting 6.00 M stock solutions. 1 What volume of 6.00 M stock solurion and whar volume of water is required to prepare 50.0 mL of 1.0 M solution? mL H.O mL 6.00 M Stock Solution How many moles of solute are contained in 50.0 mL of 1.0 M solution? b. 2500 mL of 1.00 M HNO, (initial temperature 22.4) are mixed with 50.0 mL of 1.00 M sodum ydroide (initial temperature 21.2) in a Styrofoam calorimeter. The mass of the resulting sodium nitrate solution was 100.120g Temperanure readings after mixing were: 1 min-28.6 2 min-28.2 3 min-27.8 4 min-27.4 5 min-27.0C Denermine the average initial temperature. Average Initial Temperature Constract a temperature-time graph, and extrapolate back to zero time to determine the final temperarure. Then calculate the moles of the aqueous sodium nitrate formed, the beat fow for this quantity, and the enthalpy change in kjoules to form ONE MOLE of aqueous sodium nitrate. [SIGNS!] Appendix: The Graph-A Data Analysis Tool b k/mole AH 9= moles formed Write the balanced THERMOCHEMICAL equation for the reaction. c. When 3.890 g of solid sodium nitrate are dissolved in 50.00 g of water in a Sevrofoam calorimeser to form 53.89 g of aqueous sodium nitrate, the temperature decreases by 3.5 degrees. Determine the beat Bow (a) for this mass of solid, and then calculate the enthalpy change in kjoules for dissolving ONE MOLE of solid [SIGNS!] [NaNO, - 84.995 g/mol) 3. kl/mole AH- q= Write the balanced THERMOCHEMICAL equation for this reaction. a. What is the balanced THERMOCHEMICAL equation for the reverse reaction b. The echaipies of formation of aqueous sodium hydroxide, aqueous nitric acid, and water are 4701 k/mole, -207.4 kJ/mole, and -285.8 kJ/mole respectively (Reactions 3, 4, and the re- e of 5). Use these values, your answers from questions 2 and 3, and the balanced thermo- cbemical equations to calculate the enthalpy of formation of solid sodium nitrate in kJ/moles per ale of sodium nitrate by the algebraic summation method (HESS LAW) described earlier in the experimental discussion. 1. NOH HNO NaNO 3(a) + H2O kJ/mol 3(aq) ag 2 NENO, NANO30) kJ/mol aq -470.1 kJ/mol 3. Na, Os H2iNaO (ag) 2g) 2(g) -207.4 kJ/mol H N2)+ 1% O2g) HNO3(a) 4. +285.8 kJ/mol 5. H.O,Hg+ O2(g) kJ/mol Calculations

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