C. DETERMINATIONMass of empty calorimeter cupsMass of calorimeter cups - H₂OMass of waterMass of anhydrous MgSO (s)Moles of anhydrous MgSO (s)Calculations:Temperature Readings, 'CInitial (0)½ minute1 minute1½ minutes2 minutes3 minutes4 minutes4½ minutesOF MOLAR HEAT OF SOLVATION4.60343.91034.241 82.0090.017 mol5 minutes5½ minutes6 minutes6½ minutes7 minutes7½ minutes8 minutes8½ minutes9 minutes20.60⁰°C20.60°C20.60°C20.60°C20.60°CAdd MgSO, to water25.50°C25.90°C26.00° C26-10° C26.20° C26.30° C26.30°C26.30°C26.30° C26-30°C26.30°C Initial temperature (2 minutes)Highest temperature attained (4-9 minutes)Change in temperature, ATHeat absorbed by H.O.qHeat released by solvation ofanhydrous MgSO,, qMolar Heat of Solvation, AHCalculations:'CJ/mole1. Solid anhydrous MgSO, is very hydroscopic. When exposed to moist air it will pick up water to formMgSO, XH,O. What is the classification of compounds formed by salts containing H₂O molecules intheir crystal lattice structure?2. Relating to question 1, how might you remove the water from MgSO, XH,O?3. MgSO, XH,O can be purchased "over the counter." What is the "common" name for MgSO, XH,O?

Note: We are authorized to answer one question at a time, since you have not mentioned you are…

C. DETERMINATION OF MOLAR HEAT OF SOLVATION 4.603 Mass of empty calorimeter cups Mass of calorimeter cups - H₂O Mass of water Mass of anhydrous MgSO (s) Moles of anhydrous MgSO (s) Calculations: Temperature Readings, 'C Initial (0) ½ minute 1 minute 1 ½ minutes 2 minutes 3 minutes 4 minutes 4½ minutes 5 minutes 5½ minutes 6 minutes. 6½ minutes. 7 minutes 7½ minutes 8 minutes 8½ minutes 9 minutes 43.910 34.241 2.009 0.017 -8 -8 mol 20.60˚C 20.00°C 20.60°C 20.60°C 20.6.0°C Add MgSO, to water 25.50°C 25.90°C 26.00° C 26.10 C 26.20° C 26.30° C 26.30°C 26.30°C 26.30 C 26.30°C 26.30°C

C. DETERMINATION OF MOLAR HEAT OF SOLVATION 4.603 Mass of empty calorimeter cups Mass of calorimeter cups - H₂O Mass of water Mass of anhydrous MgSO (s) Moles of anhydrous MgSO (s) Calculations: Temperature Readings, 'C Initial (0) ½ minute 1 minute 1 ½ minutes 2 minutes 3 minutes 4 minutes 4½ minutes 5 minutes 5½ minutes 6 minutes. 6½ minutes. 7 minutes 7½ minutes 8 minutes 8½ minutes 9 minutes 43.910 34.241 2.009 0.017 -8 -8 mol 20.60˚C 20.00°C 20.60°C 20.60°C 20.6.0°C Add MgSO, to water 25.50°C 25.90°C 26.00° C 26.10 C 26.20° C 26.30° C 26.30°C 26.30°C 26.30 C 26.30°C 26.30°C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Use the data table below, complete only Reaction B of the Post Lab Questions.
Pre-Laboratory Schematic Diagram:Please create a schematic diagram of Constant Pressure Calorimetry. Thank you!
A stude. right). as two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at thermometer stirrer First, a 7.500 g tablet of benzoic acid (C,H,CO,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 17.00 °C to 57.08 °C over a time of 15.0 minutes. Next, 4.440 g of ethane (C,H,) are put into the "bomb" and similarly completely burned in an excess of oxygen. This olo time the temperature of the water rises from 17.00 °C to 62.17 °C. chemical reaction "bomb" Ar Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 20,H, (g) + 70,(g) 4Co,g) + 6H,0 () Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for…
1-23.4 2-29 3-26.3 4-24.3 5-19.6
View Available Hint(s) ? ΔΗ Admol hemistry.com/myct/itemView?assignmentProblemID-174388852 acer
Please answer all, no need for explanation I will rate your answer thank you
Calorimetery practical 7: Q= Calculate the enthalpy of neutralization for ( in units of kJ/mol H2O formed ) for both HCl and HAc. Use all parts : a, b and c. [Must use the normal equation and equation: (Specific heat capacity of water x mass of water x change in temp of water ) / (mass of metal x change in temp of water )] Part A Mass of metal (g) - 10.254 Temperature of boiling water bath (°C) 100.4 Mass of calorimeter (g) 4.044 Mass of calorimeter and water (g) 20.519 Time-zero from graph (s) 45.0 Initial temperature of water from graph(°C) 22.3 Final temp = 29.2 Equation of extrapolation curve from graph- y = –0.0047291x + 29.2 Part B Molarity of NaOH (M) 1 Molarity of HCl (M) 1.1 Mass of calorimeter (g) 3.403 Volume of HCl (mL) 50.0 Volume of NaOH (mL) 50.0 Time-zero from graph (°C) 35.5 Initial temperature of mixture from graph(°C) 22.2 Final temperature 29.3 Equation of extrapolation curve from graph y = –0.0017787x + 29.3 Mass of calorimeter and mixture (g)…
A solution is made by mixing 287.0 mL287.0 mL of ethanol initially at 13.1 ∘C13.1⁢ ∘C with 287.0 mL287.0 mL of water initially at 22.0 ∘C22.0⁢ ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL0.789 g/mL and the density of water is 1.00 g/mL1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C4.184 J/g·°C.
Please answer correct significant figu
Calculate the DH0of the following reaction N2H4 (s) + 2H2O2 (s) ---> N2 (g) + 4 H2O (s) N2H4 (s) + O2 (g) ---> N2 (g) + 2H2O (s) DH0 = -622.2 kj H2 (g) + ½ O2 (g) ---> H2O (s) DH0= -285.8 kj H2 (g) + O2 (g) ---> H2O2 (s) DH0= -187.8 kj
Please help with questions 5-12. Note: mass of HCl solution = 50.0g and mass of NaOH solution = 50.0g
b) Construct an enthalpy cycle and calculate the enthalpy of combustion in each case using the above data. 3. Given the following data: AH(CH4) = -74.8 kJmol-¹, AH(CH3CI) = -134.5 kJmol-¹, AH (HCI) = -92.3 kJmol-¹; Construct an enthalpy cycle and calculate H for the reaction CH4(g) + Cl2(g) CH3CI(g) + HCl(g) 4. Given the data: 4NH3(g) + 302(g) 0 2N2(g) + 6H2O(1), AH = -1530kJmol-1 H2(g) + 1/2O2(g) □ H₂O(1), AH = -288 kJmol-¹ Construct an enthalpy cycle and calculate the enthalpy of formation of ammonia.