Chapter 5: Enthalpy of a Reaction.. I04/08/20 CORE out of 21 How would you combine reactions A-C, shown below, to obtain the overall reaction: NH, (g) + BH, (g) +0,(g) 2H,0(g) + HBNH(s) Please select all that pply. A. 2H, (g) + 0,(g) → 2H,0(g) B. H;BNH, (s) → NH,(g)+BH, (g) C. H,BNH, (s) → 2H, (g) + HBNH(s) Choose one or more: 4 OF 17 QUESTIONS COMPLETED 0247 O Type here to search F1 F2 F3 F4 F5 F6 F7 F8 F9 %24 & 8. Lnt O https://cligital.wwnorton.com 30952 4. 04/08/20 < Chapter 5: Enthalpy of a Reaction... OUT OFRA H,BNH, (s) → 2H, (g) +HBNH(s) Choose one or more: O A. reverse C O B. multiplyA by 2 O C. reverse B O D. divide B by 2 OE. add resulting equations together O F. reverse A O G. divide A by 2 H. multiply B by 2 O 1. multiply C by 2 O J. divide C by 2 4 OF 17 QUESTIONS COMPLETED O Type here to search F2 F3 F4 F5 F6 F7 F8 F9 #3 24 &

Chapter 5: Enthalpy of a Reaction.. I04/08/20 CORE out of 21 How would you combine reactions A-C, shown below, to obtain the overall reaction: NH, (g) + BH, (g) +0,(g) 2H,0(g) + HBNH(s) Please select all that pply. A. 2H, (g) + 0,(g) → 2H,0(g) B. H;BNH, (s) → NH,(g)+BH, (g) C. H,BNH, (s) → 2H, (g) + HBNH(s) Choose one or more: 4 OF 17 QUESTIONS COMPLETED 0247 O Type here to search F1 F2 F3 F4 F5 F6 F7 F8 F9 %24 & 8. Lnt O https://cligital.wwnorton.com 30952 4. 04/08/20 < Chapter 5: Enthalpy of a Reaction... OUT OFRA H,BNH, (s) → 2H, (g) +HBNH(s) Choose one or more: O A. reverse C O B. multiplyA by 2 O C. reverse B O D. divide B by 2 OE. add resulting equations together O F. reverse A O G. divide A by 2 H. multiply B by 2 O 1. multiply C by 2 O J. divide C by 2 4 OF 17 QUESTIONS COMPLETED O Type here to search F2 F3 F4 F5 F6 F7 F8 F9 #3 24 &

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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We can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO2 (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO2 (+33.18 kJ/mol) to derive the enthalpy change for this reaction.
A model for the compound 2-ethylbutanoic acid is shown. ball & stick Ⓒ+ labels [References] Use the References to access important values if needed for this question. Write a balanced chemical equation that shows the formation of 2-ethylbutanoic acid from the elements carbon (C), hydrogen (H₂ ) and oxygen (O₂). (Use the smallest integer coefficients possible and do not include states. Enter the elements in the order: C, H, then 0 in the product box.) Submit Answer + + Retry Entire Group - 9 more group attempts remaining Previous Next Save and Exi
Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ Use Reaction 2. How much energy (in kJ) is released when 79.0 g of oxygen difluoride decomposes?
Consider the reaction of a mixture of NaHCO3 and Ca(HCO3)2 with excess HCl. The net ionic reaction observed is H+(aq) + HCO3-(aq) → H2O(l) + CO2(g) The data for this problem is for 25 oC 7.701 g of a sample containing a mixture of NaHCO3 and Ca(HCO3)2 is mixed with an excess of HCl to produce CO2 gas. When all of the (dried) gas is collected in a 1.00 L vessel, the total pressure is 1.452 atm. How many g of NaHCO3 were present in the initial sample?
Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) → H,0(g) AH1 = -241.8 kJ 2) X(s) + 2 Cl,(g) → XCl,(s) AH2 = +475.9 kJ 3) H,(g) + CL,(g) HCl(g) АНз 3 —92.3 kJ → 4) X(s) + O,(g) –→ XO,(s) AH4 = -748.7 kJ 5) Н, О(2) — н,00) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)
The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1 J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO₂(g) + 11H₂O(l) → C12H22 O11 (8) + 1202 (9) AH = 5640 kJ calculate the percentage of sunlight used to produce the sucrose - that is, determine the efficiency of photosynthesis in this field. Percent efficiency = %
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The combustion of propane gas (C3H8; molar mass = 44.09 g/mol) occurs according to the following equation: C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) Given the following standard molar enthalpy of formation (DHof), how much energy in kilojoules is produced when 1.00 g of propane is completely combusted? DHof[C3H8] = -103.8 kJ/mol; DHof[CO2] = -393.5 kJ/mol, and DHof[H2O(g)] = -241.8 kJ/mol (A) 2043.9 kJ (B) 531.5 kJ (C) 12.1 kJ (D) 46.4 kJ
The conversion of natural gas, which is mostly methane,into products that contain two or more carbon atoms, suchas ethane (C2H6), is a very important industrial chemicalprocess. In principle, methane can be converted into ethaneand hydrogen: 2 CH4(g)----->C2H6(g) + H2(g) In practice, this reaction is carried out in the presence ofoxygen: 2 CH4(g) + 12O2(g)---->C2H6(g) + H2O(g) (a) Calculate K for these reactionsat 25 °C and 500 °C. (b) Is the difference in ΔG° forthe two reactions due primarily to the enthalpy term (ΔH)or the entropy term 1-TΔS2? (c) Explain how the precedingreactions are an example of driving a nonspontaneousreaction, (d) The reaction of CH4 and O2 to form C2H6 and H2O must be carried out carefully to avoid a competingreaction. What is the most likely competing reaction?
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Given the enthalpy of formation data in the table below, what is the enthalpy of reaction for the reaction you performed in this lab? How does this compare to your experimental results? To calculate the enthalpy of reaction, use the formula below. AHran=EAH; (products) - EAH; (reactants) ΔΗ, Note that you will need the balanced chemical equation for the reaction performed in the lab, which can be found in the Background in your Hayden-McNeil course site. Also note that AHⓇ for standard state elements is 0 kJ/mol. Substance AH₁ (kJ/mol) MgCl₂(aq) -785.1 kJ/mol HCl(aq) -167.2 kJ/mol