1. Using bond energies, calculate ΔH for the reaction below.
CH4(g) + Cl2(g) + F2(g) ---- CF2Cl2(g) + HF(g) + HCl(g)
2. Which of the following likely to be more soluble in water? Circle your pick.
a) C6H12 or C6H12O6 Explain:
b) CH3CH2COOH or CH3CH2COONa Explain:
c) HCl or acetic CH3CH2Cl Explain:
1. Using bond energies, calculate ΔH for the reaction below. CH4(g) + Cl2(g) + F2(g)...
Use the bond energies below to estimate AH for the following reaction: CH4 (g) + Cl2 (g) - CH3CI (g) + HCl (g) Bond Energies (kJ/mole) single bonds. multiple bonds H C. Cl H. 432. C=O 799 C. 412. 346. C=C.602 O. 459. 358. 142 C=C 835 Cl 431. 328. 242. O=O 494
OTHERMOCHEMISTRY Calculating the heat of reaction from bond energies Calculate the heat of reaction AH for the following reaction: 2 HCl(g) + F2(9)-2 HF(g) + Cl2(9) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ Х 5 ? mol
Use the bond energies provided to estimate ΔH°rxn for the reaction below.PCl3(g) + Cl2(g) → PCl5(l)ΔH°rxn = ?BondBond Energy (kJ/mol)Cl-Cl243P-Cl331
1a. Using bond dissociation energies, calculate the heat of reaction (ΔH) for the reaction shown below. Show all your work and provide a reference for where you got your bond dissociation energy values. 1b. Is this reaction endothermic or exothermic? Explain. Provide energy diagrams showing the two processes. Circle the one that corresponds to this reaction. Label the axis appropriately as well as the activation energy (Ea). la. Using bond dissociation energies, calculate the heat of reaction (AH) for the...
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
Using the Table of Bond Energies in CH 11.5 calculate the ΔH for : H2(g) + F2(g) → 2HF(g) assume: H-H ; F-F ; H-F bonds A. -543 B. -24 C. 24 Given: A(g) + B(g) → D(g) ; ΔH = 56kJ/mol ; the enthalpy change for 2A(g) + 2B(g) → 2D(g) is: A. -56 B. -112 C. 112 Given: A(g) + B(g) → C(g) ΔH = 10kJ/mol ; C(g) → D(g) ΔH = 30kJ/mol; the ethalpy change for: A(g)...
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) Calculate ΔH for the reaction using the bond enthalpies given. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Calculate the overall enthalpy change for this reaction using the bond enthalpies given.
please do not answer Using the bond energies provided below, calculate DH° for the reaction CH4(g) + 4C12(8) --> CC14(g) + 4HCI(g) Show calculation set-up. Bond: C-H CI-CI C-ci HCI Bond energy (kJ/mol): 413 243 339 427 O-110 kJ E) 440 kJ - 440 kJ 1422 k) O 110 kJ
Using the table of bond energies below, calculate the following enthalpy values associated with this reaction: 2 HF (g) H2 (g)F2 (g) Bond type Bond Energy (kJ/mol) 159 F-F H-H 432 H-F 565 Enter your answers to zero decimal places. Ignore significant figure rules. Include negative signs if necessary What is the sum of the reactant bond enthalpies? kJ What is the sum of the product bond enthalpies? kJ What is the overall enthalpy of reaction? kJ