None Use the References to access important values if needed for this question.For the reaction below:CH₂CH₂-CIH-NH2CH3CH2-NH2H-CIa. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data fromyour text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign andunits.b. Is the reaction exothermic or endothermic?c. Is the reaction likely to proceed spontaneously in the direction written? ©Submit AnswerRetry Entire Group3 more group attempts remaining

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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 41QAP: The enthalpy change for the reaction of hydrogen gas with fluorine gas (o produce hydrogen fluoride...

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Calculate the enthalpy of reaction for HCN(g)H(g)+C(g)+N(g) from enthalpies of formation (see Appendix C). Given that the CH bond enthalpy is 411 kJ/mol, obtain a value for the CN bond enthalpy. Compare your result with the value given in Table 9.5.
Which statement(s) is/are true about bond enthalpy? (a) The bond energy for a triple bond between A and B is three times that of a single bond between A and B. (b) H for the breaking of a bond is always a negative number. (c) Energy is required to make a bond. (d) Bond enthalpy is defined only for bonds broken or formed in the gaseous state. (e) The presence of bonds does not influence the geometry of a molecule. However, the presence of bonds affects the value of the bond enthalpy between two atoms.
The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?
Calculate the standard heat of formation of the compound ICl(g) at 25C. (Hint: Use Table 8.5 and Appendix 4 data.)
Calculate the standard molar enthalpy of formation of NO(g) from the following data: N2(g)+2O22NO2(g)H298=66.4kJ2NO(g)+O22NO2(g)H298=114.1kJ
The enthalpy change for the reaction of hydrogen gas with fluorine gas (o produce hydrogen fluoride is 542 U for the equation as written: mg src=Images/HTML_99425-10-41QAP_image001.jpg alt="" align="top"/> l type='a'> What is the enthalpy change per mole of hydrogen fluoride produced? Is the reaction exothermic or endothermic as written? What would be the enthalpy change for the reverse of the given equation (that 1%, for the decomposition of HF into its constituent elements)?
You will not find “hydroxide” in the stockroom, but you will find sodium hydroxide (NaOH) andpotassium hydroxide (KOH). Lithium hydroxide (LiOH) is expensive and used in spacecraft airfilters since hydroxide reacts with carbon dioxide, and lithium is lighter than sodium or potassium.Cesium and francium hydroxides are very expensive and little used. Is this information consistentwith your answer to the previous question?
Compare your answer from Exercise 72 of Chapter 3 to the H value calculated from standard enthalpies of formation in Appendix 4. Explain any discrepancies. .. 72. Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond engines(Table 3-3) to estimate E for this reaction
Draw a curve that describes the energy of a system with H and Cl atoms at varying distances. Then, find the minimum energy of this curve two ways. (a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?) (b) Use the enthalpy of reaction and the bond energies for H2 and Cl2 to solve for the energy of one mole of HCl bonds. H2(g)+Cl2(g)2HCl(g)Hrxn=184.7kJ/mol
Oxygen atoms can combine with ozone to form oxygen: O3(g) + O(g) 2 O2(g) rH = 392 kJ/mol-rxn Using rH and the bond dissociation enthalpy data in Table 8.8, estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, O3. How does your estimate compare with the energies of an OO single bond and an O=O double bond? Does the oxygen-oxygen bond dissociation enthalpy in ozone correlate with its bond order?
If a reaction occurs readily but has an endothermic heat of reaction, what must be the driving force for the reaction?
Enthalpy changes for the following reactions can be determined experimentally: N2(g) + 3 H2(g) 2 NH3(g) rH = 91.8 kJ/mol-rxn 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) rH = 906.2 kJ/mol-rxn H2(g) + O2(g) H2O(g) rH = 241.8 kl/mol-rxn Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that cannot be measured directly because the reaction is reactant-favored). N2(g) + O2(g) NO(g) rH = ?

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