Part A Below is an Arrhenius plot for the isomerization of cyclopropane to propene, showing the equation for the linear best fit to the data. Arrhenius Plot for the Isomerization of Cyclopropane What are the units for the slope of this line? -1 -2 -3 -4 14622x +22.008 °C K K-1 -10 0.0015 0.0016 0.0017 0.0018 0.0019 0.0020 0.0021 0.0022 Submit Request Answer T-/K-1

Part A Below is an Arrhenius plot for the isomerization of cyclopropane to propene, showing the equation for the linear best fit to the data. Arrhenius Plot for the Isomerization of Cyclopropane What are the units for the slope of this line? -1 -2 -3 -4 14622x +22.008 °C K K-1 -10 0.0015 0.0016 0.0017 0.0018 0.0019 0.0020 0.0021 0.0022 Submit Request Answer T-/K-1

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction

Section: Chapter Questions

Problem 2ASA

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Use the standard reaction energies given below to determine DeltaG^°rxn for the following reaction: 2XO2(g) —> 2XO(g) + O2(g) From the standard reaction energy of X2(g) + O2 —> 2XO(g) DG^°= 155.52 Kjxmol-1 X2(g) + 2O2 —> 2XO2(g) DG^°= 168.55 Kjxmol-1 Given answer in Kj/mol. Give answer to two decimal places.
The reaction is carried out with [PCl5]i =0.40M at 25°C PCl5(g)⇌PCl3(g)+Cl2(g) K=0.00105 Use the small x approximation and "test x." Report the percent, to two decimal places, when testing x.
Use the data provided below to estimate (a) the temperature at which CaCO3 decomposes spontaneously assuming ΔrH and ΔrS remain unchanged at the temperature region of interest. CaCO3 (s) --> CaO (s) + CO2 (g) ΔfHo -1207 -635 -394 kJ mol-1 Smo 93 40 214 J K-1 mol-1 Tspont. >= ________ K. 3 s.f.
Compound Δ?∘f (kJ/mol)Δ⁢Gf∘ (kJ/mol) A +387.7+387.7 B +600.4+600.4 C +402.0+402.0 Use the data given here to calculate the values of Δ?∘rxnΔ⁢Grxn∘ at 25 ∘25⁢ ∘C for the reaction described by the equation A+B↽−−⇀C A+B↽−−⇀CA+B↽−−⇀C Δ?∘rxn=Δ⁢Grxn∘= kJkJ If Δ?∘rxnΔ⁢Hrxn∘ and Δ?∘rxnΔ⁢Srxn∘ are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the left. enthalpy-driven to the right. entropy-driven to the right. entropy-driven to the left.
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ in the combustion of ethane in the presence of excess oxygen yields carbon dioxide and water: 2C2H2(g) + 7O2(g) → 4CO2(g) + 6H2O(l) in J/K?
Calculate the Ksp for the dissociation of solid barium nitrate in water at 25.0 oC. The ΔGo for Ba(NO3)2(s) = -797 kJ/mole. Ba(NO3)2(s) ↔ Ba+2(aq) + 2NO3-1(aq) Group of answer choices 4.47x10-23 5.06x10-4 1.97x103 5.22x10-40 2.24x1022 0.992
Consider the problem below: (Equation 1) 2 H2O(l) ---> 2 H2(g) + O2(g) ΔH = 571.6 kJ (Equation 2) N2O5(g) + H2O(l) ---> 2 HNO3(l) ΔH = -73.7 kJ (Equation 3) 2 H2(g) + 6 O2(g) + 2 N2(g) ---> 4 HNO3(l) ΔH = -696.4 kJ (Equation 4) 2 N2(g) + 5 O2(g) ---> 2 N2O5(g) ΔH = ??????? To find ΔH for equation 4 you must:
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Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 C2H4(g) 52.30 68.11 219.4 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ for the catalytic hydrogenation of acetylene to ethene, C2H2(g) + H2(g) → C2H4(g) inJ/K?
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