8 An energy cycle is drawn for the following reaction. Br₂(1) + 3F₂(g) → 2BrF3(1) +698kJ 2Br(g) + 6F(g) 2BrF3(g) 2BrF3(1) Br₂(l) + 3F₂(g) The standard enthalpy of formation of BrF3(1) = -301 kJ mol-¹. The enthalpy change of BrF3(1) to BrF³(g) is +44 kJ mol¯¹. What is the average bond energy of the Br-F bond in BrF3? 152 kJ mol-¹ B 202 kJ mol-¹ C 304 kJ mol-¹ A D 404 kJ mol-¹

8 An energy cycle is drawn for the following reaction. Br₂(1) + 3F₂(g) → 2BrF3(1) +698kJ 2Br(g) + 6F(g) 2BrF3(g) 2BrF3(1) Br₂(l) + 3F₂(g) The standard enthalpy of formation of BrF3(1) = -301 kJ mol-¹. The enthalpy change of BrF3(1) to BrF³(g) is +44 kJ mol¯¹. What is the average bond energy of the Br-F bond in BrF3? 152 kJ mol-¹ B 202 kJ mol-¹ C 304 kJ mol-¹ A D 404 kJ mol-¹

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...

See similar textbooks

Similar questions

Determine the change in enthalpy (kJ/mol) for the following reaction. Use significant figures CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) H=?
Given that 2Al(s) + 3 2 O2(g) → Al2O3(s) Δ H o rxn = −1601 kJ/mol and 2Fe(s) + 3 2 O2(g) → Fe2O3(s) Δ H o rxn = −821 kJ/mol calculate the standard enthalpy change for the following reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) Enter your answer in scientific notation. × 10 kJ
What is the enthalpy change for the first reaction? Fe2O3(s) → 2Fe(s) + 3/2O2(g) ΔH = 4Fe(s) + 3O2(g) → 2Fe2O3 (s) ΔH = -1,652 kJ
enon 19 of 23 For the chemical reaction Ca (s) + % O2 (g) What is the enthalpy for the reaction 2 CaO (s) → 2 Ca (s) + O2 (g)? CaO (s) AH° = -635 kJ/mol.
+ (3)CHN O2(g) NO(g) + H2O(g) --> -- -- Based on the enthalpies of formation, how much energy, in kJ, will be released when 6.46 grams of H2O(g) are produced?
4. Determine the enthalpy of formation for Lithium Oxide given the three equations below: 2Li(s) + ¹0₂(g) → Li₂0(s) AH = Unknown Li(s) + H₂O(l) → LiOH(aq) + ½H₂(g) Liz0(s) + H20() → 2LiOH(aq) H₂(g) + 1/2O₂(g) H₂O(l) AH = -222.7 kJ AHⓇ = -133.3 kJ ΔΗ = -285.8 kJ
Cl2 (g) + H2 (g) → 2 HCl (g) ΔH0rxn = ‒184.6 kJ 9. What is the formation reaction of HCl (g)? Group of answer choices A.No answer text provided. B.2 HCl (g) → Cl2 (g) + H2 (g) C.½ Cl2 (g) + ½ H2 (g) → HCl (g) D.HCl (g) → ½ Cl2 (g) + ½H2 (g) E.Cl2 (g) + H2 (g) → 2 HCl (g)
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
For the reaction below ΔH = -296 kJ per mole of SO2 formed. S(s) + O2(g) → SO2(g) (c) What quantity of energy is required to break up exactly 2 mol of SO2(g) into its constituent elements?
A) Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g)2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘f=33.2 kJ mol−112N2(g)+O2(g)→NO2(g), ΔHf∘=33.2 kJ mol−1 12N2(g)+12O2(g)→NO(g), ΔH∘f=90.2 kJ mol−112N2(g)+12O2(g)→NO(g), ΔHf∘=90.2 kJ mol−1 B) Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s)4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘rxn=+2035 kJ mol−1B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔHrxn∘=+2035 kJ mol−1 2B(s)+3H2(g)→B2H6(g), ΔH∘rxn=+36 kJ mol−12B(s)+3H2(g)→B2H6(g), ΔHrxn∘=+36 kJ mol−1 H2(g)+12O2(g)→H2O(l), ΔH∘rxn=−285 kJ mol−1H2(g)+12O2(g)→H2O(l), ΔHrxn∘=−285 kJ mol−1 H2O(l)→H2O(g), ΔH∘rxn=+44 kJ mol−1
Small amounts of oxygen gas can be produced in the laboratory by heating potassium chlorate, KClO3. Determine the enthalpy change for this reaction using known enthalpies of formation. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
Given the reactions and the heats of reaction associated with them, use Hess' Law to calculate the heat of formation of SO2(g). S(s) + 3/2 O2(g) → SO3(g) ΔH = -395 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH = -198 kJ