5.(a) Nitrogen reacts with fluorine to form nitrogen trifluoride, NF3. (i) The chemical equation can be represented as shown. NEN + 3 F-F → 2 F-N-F Some bond energies are shown in the table. bond bond energy in kJ/mol NEN 945 F-F 160 N-F 300 Calculate the energy change for the reaction between nitrogen and fluorine, using the following steps: • energy taken in to break bonds kJ • energy released when bonds are formed kJ

5.(a) Nitrogen reacts with fluorine to form nitrogen trifluoride, NF3. (i) The chemical equation can be represented as shown. NEN + 3 F-F → 2 F-N-F Some bond energies are shown in the table. bond bond energy in kJ/mol NEN 945 F-F 160 N-F 300 Calculate the energy change for the reaction between nitrogen and fluorine, using the following steps: • energy taken in to break bonds kJ • energy released when bonds are formed kJ

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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The table below includes the bond enthalpy (the energy required to separate the diatomic molecule into its atoms) and the bond length for each diatomic molecule. Diatomic Molecule Bond Enthalpy (kJ/mol) Bond Length (pm) Cl2 243 199 O2 498 121 N2 945 110 Identify the observed trend between bond enthalpy and number of shared electrons: as the number of electrons shared between two atoms increases, the bond enthalpy ( increases / decreases / remains unchanged ). Identify the observed trend between bond length and number of shared electrons: as the number of electrons shared between two atoms increases, the bond length ( increases / decreases / remains unchanged ).
Using the bond energies provided below, calculate the enthalpy change (AHrxn) for the reaction shown. 2H₂O (g) → 2H2(g) + O2(g) Bond: Avg. bond energy (kJ/mol): -425 kJ/mol -509 kJ/mol 356 kJ/mol 509 kJ/mol 7 kJ/mol 425 kJ/mol H-H O-H 432 467 O-O 146 O=O 495
7. Consider the following compounds: BaBr 2, MgCl 2, and SrCl 2. Answer the following questions based on expected periodic trends: (a) Which is expected to have the shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?
1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): Rbl, CaO, SrO, NaCl 1b)Rank the following elements in order of increasing metallic character (from least metallic to most metallic): Ca, S, Rb, Ar, Se 1c) by using the attached table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2N-NH2 + O2 ---> N2+ 2H2O
Use the bond energies (kJ/mol) given (using variables only) to calculate the total enthalpy (energy) change for the following reaction: H2C=CH2(g) + Cl2(g) = ClH2C-CH2Cl(g) (Each carbon in the product has 2 H and one Cl atom bonded to it) Bond Energies: C-H: A C=C: B Cl-Cl: C C-C: D C-Cl: E
1. Hydrogen (H2) and oxygen (O2) react to produce water (H2O). (a) Write down the equation for the above reaction. (b) The enthalpy change of reaction is –286 kJ mol-!. Is the reaction endothermic or exothermic? (c) What kinds of bonds are broken during the reaction? (d) What kinds of bonds are formed during the reaction? (e) Construct a diagram showing the change in enthalpy for the reaction.
1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO 1b)Rank the following elements in order of decreasing metallic character (from most metallic to least metallic): S, CI, K, Cs, Se 1c) by using the table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2C=CH2 + Cl2 ---> Cl-CH2-CH2-Cl
3.Calculate the overall energy change in the combustion of ethane, C2H. Is it exothermic reaction or an endothermic reaction? (An example is shown in another document, which is also posted) Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391
9. Acetylene gas (C2H2) is used in welding. Use bond dissociation energies to determine the AErxn, in kJ/mol C2H2, for the reaction: 2 C2H2(g) + 5 Oz(g) → 4 CO2(g) + 2 H2O(g)
Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation CC14(g) + 2 F₂ (g) → CF₁ (g) + 2 Cl₂ (g) 2 The bonding in the molecules is shown. ΔΗ +=++· rxn = -CI F-F F-F -C-F CI-CI CI-CI Average molar bond enthalpies (Hbond) Bond Bond O-H C=N 0-0 N-H C-O N-N 0=0 N=N C=O N=N C-C F-F C=C Cl-Cl C=C Br-Br C-H H-H C-F H-F C-Cl H-Cl C-Br H-Br C-N H-S C=N S-S kJ.mol-¹ 464 142 351 502 730 347 615 811 414 439 331 276 293 615 kJ.mol-1 890 390 159 418 945 155 243 192 435 565 431 368 364 225 kJ.mol-¹
Use the bond energies from the table in the reference sheet to determine the approximate enthalpy change of the following reaction. H2(g) + Br2(g) --> 2HBr(g) Group of answer choices -57 kJ/mol -114 kJ/mol -256 kJ/mol 256 kJ/mol
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: C2(g) + F2(g)–2CIF(g) kJ