Part ACalculate the standard enthalpy change for the reactionUse the following data:SubstanceΔΗ;(kJ/mol)ABDExpress your answer to three significant figures and include the appropriate units.▸ View Available Hint(s)AH = 273Submit✓ CorrectPart B410-235-419211-519SubmitPrevious AnswersFor the reaction given in Part A, how much heat is absorbed when 3.00 mol of A reacts?Express your answer to three significant figures and include the appropriate units.► View Available Hint(s)kJmolμAkJ/molPrevious Answers* Incorrect; Try Again; 3 attempts remaining2A+B=2C+2D

Answered: Image /qna-images/answer/20ca159b-4818-4103-9c3e-1952c9a54006.jpg

Part A Calculate the standard enthalpy change for the reaction Use the following data: Substance ΔΗ, (kJ/mol) A B с D Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ΔΗ; = 273 Submit Correct Part B -235 -419 211 -519 410 kJ mol Previous Answers For the reaction given in Part A, how much heat is absorbed when 3.00 mol of A reacts? Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) = ? kJ/mol Submit Previous Answers * Incorrect; Try Again; 3 attempts remaining 2A+B=2C+2D

Part A Calculate the standard enthalpy change for the reaction Use the following data: Substance ΔΗ, (kJ/mol) A B с D Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ΔΗ; = 273 Submit Correct Part B -235 -419 211 -519 410 kJ mol Previous Answers For the reaction given in Part A, how much heat is absorbed when 3.00 mol of A reacts? Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) = ? kJ/mol Submit Previous Answers * Incorrect; Try Again; 3 attempts remaining 2A+B=2C+2D

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter10: Energy

Section: Chapter Questions

Problem 81AP

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9.50 When a 13.0-g sample of NaOH(s) dissolves in 400.0 mL of water in a coffee cup calorimeter, the temperature of the water changes from 22.6°C to 30.7C Assuming that the specific heat capacity of the solution is the same as for water, calculate (a) the heat transfer from system to surroundings and (b) H for the reaction NaOH(s)Na+(aq)+OH(aq)
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
9.57 The heat of combustion of butane is —2877 kJ/mol. Use this value to find the heat of formation of butane. (You may also need to use additional thermochemical data found in Appendix E.)
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The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?
Given the following (hypothetical) thermochemical equations: A+B2C;H=447kJA+3D2E;H=484kJ2D+B2F;H=429kJ Calculate H, in kJ, for the equation 4E+5B4C+6F
9.103 One reason why the energy density of a fuel is important is that to move a vehicle one must also move its unburned fuel. Octane is a major component of gasoline. It burns according to the reaction 2C8H18(l)+25O2(g)16CO2(g)+18H2O(g) H = 1.10104 kJ Starting from this thermochemical equation, describe how you would determine the energy density, in kJ/g, for octane. Be sure to indicate what you would need to calculate or look up to complete this problem.