What is the change in enthalpy (in kJ mol⁻¹) for the following reaction Cl₂(g) + 2LiF(s) ⇄ 2ClF(g) + 2Li(s) Question 1 options: 1) -1064 kJmol⁻¹ 2) 1123 kJmol⁻¹ 3) -1123 kJmol⁻¹ 4) 1064 kJmol⁻¹ 5) 199.65 kJmol⁻¹ How much heat is needed to convert 15.0 grams of BCl₃(s) at -107.4˚C to BCl₃(g) at 12.4˚C? Question 2 options: 1) 0.269 kJ 2) 4.95 kJ 3) 1.64 kJ 4) 3.04 kJ 5) 16.4 kJ This was all of the information given to us. Thank you!

What is the change in enthalpy (in kJ mol⁻¹) for the following reaction Cl₂(g) + 2LiF(s) ⇄ 2ClF(g) + 2Li(s) Question 1 options: 1) -1064 kJmol⁻¹ 2) 1123 kJmol⁻¹ 3) -1123 kJmol⁻¹ 4) 1064 kJmol⁻¹ 5) 199.65 kJmol⁻¹ How much heat is needed to convert 15.0 grams of BCl₃(s) at -107.4˚C to BCl₃(g) at 12.4˚C? Question 2 options: 1) 0.269 kJ 2) 4.95 kJ 3) 1.64 kJ 4) 3.04 kJ 5) 16.4 kJ This was all of the information given to us. Thank you!

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section18.4: Entropy Measurement And Values

Problem 3RC: Calculate rS for the following reaction at 25 C. 2 H2(g) + O2(g) 2 H2O() (a) 326.6 J/K mol-rxn...

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If a reaction is exergonic, which of these thermodynamic parameters is necessarily negative? A) ∆G b) ∆H c) ∆S d) ln K Which statement is always true about exergonic reactions? A) they give off heat b) they proceed very rapidly c) they have the potential of proceeding without energy input d) they require enzyme catalysis If the value of the equilibrium constant K is zero, this tells you: a) the reaction requires an enzyme b) the reaction is at equilibrium c) the reaction is endergonic d) the reaction is exergonic Which of these thermodynamic parameter are changed by enzymes? A) Gibbs free energy b) entropy c) activation energy d) all of these
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1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJ
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