Part IllI: Determine the molar enthalpy change for reaction 3 using Hess's lawHCl(aq) + NH3(aq) ® NH4CI(aq)DH3 =In the space below, show all calculation set-ups to determine the molar heat of enthalpy, inkJ/mol HCl, of reaction 3 (DH3). For full credit, all numerical answers must be rounded off to correct sig figsand with proper units. Answers without calculation set ups receive no credit.

The standard enthalpy of formation of HCl(aq) is -167.2kJ/mol. The standard enthalpy of formation of…

Answered: Part IllI: Determine the molar enthalpy…

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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When 2.232 g of AX (s) dissolves in 147.5 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 34.8 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
1.Given reactions A - C, determine the the change in enthalpy (kJ) for the reaction between C(s) + H2(g). Do not type units into your answer. C(graphite) + 2 H2(g) ⟶⟶ CH4(g) Δ?=?ΔH=? A. C(graphite) + O2(g) ⟶⟶ CO2(g) Δ?=−393.51??ΔH=−393.51kJB. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJC. CO2(g) + 2 H2O(l) ⟶⟶ CH4(g) + 2 O2(g) Δ?=890.30??ΔH=890.30kJ 2. Based on your answer to the previous problem, determine the value of q (kJ) if 5.08 grams of methane (CH4) gas is produced from graphite and hydrogen gas. Do not type units into your answer.
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
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Determine the molar enthalpy change for reaction 3 using Hess’s law HCl(aq) + NH3(aq) ® NH4Cl(aq) DH3 = A. In the space below, show all calculation set-ups to determine the molar heat of enthalpy, in kJ/mol HCl, of reaction 3 (DH3). All numerical answers must be rounded off to correct sig figs and with proper units. If the true value of DH3 is –52.2 kJ/mol, calculate the percent error. Round off the answer in correct sig figs.
Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
Calculate the enthalpy of formation of 1 mole SO₂(g) from the standard enthalpy changes of the following reactions: 2SO3(g)2SO₂(g) + O₂(g) 2S (s) +30₂(g) → 2SO3(g) →→ SO₂(g) S(s) + O₂(g) kJ ΔΗ AH rxn 1=+196 kJ rxn 2 = -790 kJ AHO rxn 3 = ? k
CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = ____kJ(c) If the enthalpy change is 18.0 kJ, how many grams of hydrogen gas are produced?____g(d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = ____kJ(e) Calculate E when 750.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K _____kJ HopHelpCh5N1
When 0.215 g of sodium metal is added to an excess of hydrochloric acid, 2230 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HC1(aq) 2 NaCI(aq) + H, (g) Enthalpy of reaction: kJ
Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g) C4H10(9) (2) C₂H4(g) →→2C(s) + 2H₂(g) (3) 2C₂H4(g) + H₂(g) C4H10 (9) ΔΗ° = -125.6 kJ what is the standard enthalpy change for the reaction: KJ AHO = -52.3 kJ ΔΗ° = ?
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
Part III: Determine the molar enthalpy change for reaction 3 using Hess’s law HCl(aq) + NH3(aq) ® NH4Cl(aq) DH3 = A. In the space below, show all calculation set-ups to determine the molar heat of enthalpy, in kJ/mol HCl, of reaction 3 (DH3). For full credit, all numerical answers must be rounded off to correct sig figs and with proper units

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