se/3594/report/69138 #tab=REPORTRTeport Submission - ThermochemistryPart B data and calculationsAssigned saltMass of dry, empty calorimeter (g)Final mass of calorimeter and mixture (g)Mass of solution (g)Initial temperature (°C)Final temperature (°C)Change in temperature of solution (°C)arxn(J)(report the appropriate sign)Mass of salt (g)Moles of salt (mol)Enthalpy of Dissolution (J/mol)Enthalpy of Dissolution (kJ/mol)Dubon Reina, Sam (CDT)dubonres@myumanitoba.caTable viewList viewMeasurement or CalculationNaCl25.32127.12101.822.121.6-0.5212.833.000.051

Part 2: Explanation:Step 1: Convert heat change from J to kJ.Given that 1 kJ = 1000 J, we divide the…

Answered: se/3594/report/69138 #tab=REPORT RT…

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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Background-info: https://drive.google.com/file/d/1G7sPTuESIgWk9wpRdqAnFcsBmOlbBfLv/view?usp=sharing Question: Select each of the following statements that are true in relation to the property "standard molar enthalpy of formation". It is the measurement of the enthalpy change involved in the production of one molecule of a substance. It is measured at 1 atm of pressure. It is represented by AH°f It is measured from the constituent elements in their most stable states at the given temperature.
A chemist places 1.750 g of ethanol, C2H6O, in a bomb calorimeter with a heat capacity of 12.05 kJ/K. The sample is burned and the temperature of the calorimeter increases by 4.287°C. Calculate mol ethanol, q, heat released by combustion of ethanol and AE for the combustion of ethanol in For Blank 3 kJ/mol. Answer in standard notation and for a fractional value, enter the value as 0.005525 mol, for example.
Determine the standard heat of formation and write the thermochemical equation for the product for 1 mole of phosphorous trichloride gas forming from solid white phosphorous, P4(s), and chlorine gas.
3. Given the following thermochemical equations. 2 H2(8) + Ozle) ---→ 2 H2O (1) N2Osle) + H20 (1) ----→ 2 HNO3 (1) % N2 (e) + 3/2 O2 (e) + ½ H2(g) ---→ HNO31) AH° = - 571.5 kJ AH° = -76.6 kJ AH° = -174.0 kJ Calculate the AH° for the reaction: 2 Nz(g) + 5 Ozle) → 2 N¿Os(8)
From the heats of reaction2H2(g) + O2(g) ---> 2H2O(g) DH = -483.6 kJ 3O2(g) ---> 2O3(g) DH = +284.6 kJcalculate the heat of the reaction 3H2(g) + O2(g) ---> 3H2O(g)
Mass of empty Calorimeter is 7.73g, mass of calorimeter + water is 46.875g, mass of water is 39.145g, mass of metal is 6.354g, initial temperature of metal is 100 degrees Celsius, final temperature of calorimeter is 21.5 degree Celsius, CALCULATE T(T-Final - T-Initial).
What are the assumptions that are made when performing calorimetry to determine molar enthalpies? (C:3)
Molar Masses A = 290.41 D = 250.53– 9 %3D E = 75.44 9 %3D mole mole %3D mole G = 117.05 X = 10.93 Z = 50.01 mole mole mole If 18.23 g A, according to the balanced thermochemical equation below, how much heat (in kJ) is absorbed? 5 A+6 D→ 5 Z +5G AH = 515 kJ Please input your answer to the second decimal place Type your answer...
Please calculate Ccal for both runs!
If a 3.25 L sample of pure glycerol has a mass of 4.10×10^3 g -what is the density of glycerol in g/cm^3?
NaOH(s) trial (A) NHẠNO3 (s) trial (B) Part 2: Enthalpy of dissolution a. Mass of substance dissolved (g) b. Mass of calorimeter (g) c. Mass of calorimeter + water (g) d. Mass of water (g) 0.8314 0.7985 2.114 2.179 11.9717 12.0731 e. Total mass of reactants (g) f. Initial temperature of water (°C) g. Final temperature of solution (°C) h. Change in the temperature, AT (°C) i. Moles of solid dissolved in water (mols) j. Heat lost or gained by the water, Aqm (J) k. Heat absorbed by the calorimeter, Aq. (J) I. Heat absorbed or released by the dissolving solute Aq: = Aqm+ Aqc (J) m. Enthalpy of solution, AHrxn (kJ/mol) n. Theoretical enthalpy, calculated AHrxn (kJ/mol) 18.0 18.2 30.0 13.6 o. Percent error
Use the data table below, complete only Reaction B of the Post Lab Questions.

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