4. In the experiment we plotted In(Ksp) vs 1/T. The class average data finds a straight line graph with a slope of -12406 Kelvin and an intercept of 37.88. Assuming the molar gas constant R = 8.314 J/mol/K, what are H and IS for this process Calculations for JH Calculations for IS

4. In the experiment we plotted In(Ksp) vs 1/T. The class average data finds a straight line graph with a slope of -12406 Kelvin and an intercept of 37.88. Assuming the molar gas constant R = 8.314 J/mol/K, what are H and IS for this process Calculations for JH Calculations for IS

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...

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EKS -- Assessme... O Free Article Rewrite.. Essaylyper michael CHM 1045 10 of 13 Review | Constants | Periodic Table Part A AH is an Extensive Property button within the activity, and analyze the relationship between the two reactions that are displayed The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, AH is an extensive property Using this property, calculate the change in enthalpy for Reaction 2 Click the Reaction 1. C3 Hş(g) + 502(g)→3CO2 (g) + 4H20(g), AH1 =-2043 kJ Reaction 2 5C3 Hs(g) + 2502 (g)-+15CO2(g) + 20H,O(g), AH2 =? Express your answer to four significant figures and include the appropriate units. > View Available Hint(s) ΔΗ- Value Units Submit Previous Answers Part B AH Changes sign when a hutton within the activitu and analvza the relationchin hetwoon tha two raactione that ara dienlavad Tho reaction that was on the 4:28 PM Click on tho Iprocess is reversed 3/22/2021
Chemistry If 21. cal of heat is added to 14.5 g each of sodium chloride and ethanol at 13. "C, what is the final temperature of each substance? Be sure each of your answer entries has the correct number of significant figures. Note: Reference the Phase change properties of pure substances and Conversion factors for non-SI units tables for additional information Part 1 of 2 Final temperature of sodium chloride- Part 2 of 2 Check -0% Final temperature of ethanol- CL.P X 5 5 MacBook Air Save For Later db Submit Assignment
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A bomb calorimeter is loaded with 1.465 g of caffeine (CgH1002N4; 184.19 g/mol) brated heat capacity of the ature was 23.50 °C. The and pressurized with excess oxygen. The previously calorimeter and contents is 3550 J/°C. The initial teu known internal energy of combustion of caffeine is -4251.4 kJ/mol. What is the final temperature after combustion? Report the temperature in °C with two decimal places but do not put units in the answer box.
From the following vapor pressure data for diethyl ether, an estimate of the molar heat of vaporization of C2H5OC2H5 is P, mm Hg T, K kJ/mol. 100. 262 400. 291 Submit Answer Retry Entire Group 7 more group attempts remaining
27 of 42 (> Constants | Periodic Table A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Consider the reaction C12 H22O11 (s) + 1202(g)-12CO2(g) + 11H2O(1) in which 10.0 g of sucrose, C12 H22011, was bumed in a bomb calorimeter with a heat capacity of 7.50 kJ/C. The temperature increase inside the calorimeter was found to be 22.0°C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. q= specific heat x mass x AT Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes Express the change in internal energy in kilojoules per mole to three significant figures. 9=C x AT • View Available Hint(s) At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, gp, that is, V ΑΣφ ? AH= q, AE = kJ/mol but it is usualy expressed per mole of reactant and…
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Consider the following two-step reaction:C2H4(g) + Cl2 = C2H2Cl4(l) + H2(g) delta H = -385.76 kJ/mol C2H2Cl4(l) = C2HCl3(l) + HCl(g) Show that the overall reaction has standard heat equal to -421.017 kJ/mol using the heats of formation method.
A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. The cylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. The cylinder is also submerged in a large insulated water bath. (See sketch at right.) 1 atm pressure piston cylinder The temperature of the water bath is monitored, and it is determined from this data that 392. kJ of heat flows out of the system during the reaction. The position of the piston is also monitored, and it is determined from this data that the piston does 280. kJ of work on the system during the reaction. water bath gases O exothermic Is the reaction exothermic or endothermic? O endothermic O up Does the temperature of the water bath go up or down? O down O neither O in Does the piston move in or out? O out O neither O absorb Does the reaction absorb or release energy? O release O neither How much energy does the reaction absorb or release? Be…
Mass of eat empty calorimeter 5.10g Mass of calorimeter and HCl solution 54.29g Calculated mass of HCl solutions/₂49.699 Initial temperature of HCI Solution Initial temperature of NaOH solution Final temperature of the solution Mass of the calorimeter and solution Calculated mass of NaOH solution AT For HCl solution AT for NaOH Solution Run 1 14,2°C 20.2°C 3. The number of moles of NaOH used. 24.0°C 104.959 50.16g 4.8°C 4. The number of moles of HCI used. Show Transcribed Text Part 4: Reaction 3 NaOH(aq) + HCl(aq)→ NaCl(aq) + H₂0(1) 1. The heat energy change of the calorimeter. 104.62g 50.43д 4,0°C 3,8°C hack mittarity of the calor 3.8°C Run 2 2. The heat energy change of the HCI solution, and the heat energy change of the NaOH solution, and the total heat energy change of both solutions. 5. The enthalpy of reaction. Also calculate the average enthalpy. 5.139 54.199 49.069 20.8°C 21.00C 24.8°C