The table below shows the time-temperature course during reaction of NaOH sample of 2.02 g with 169 mL of 1M HCl. Plot the data, evaluate ΔT and calculate the reaction enthalpy. time/s t/ oC 0 19.75 15 19.80 30 19.85 45 19.89 60 19.97 75 20.02 90 19.98 105 20.13 120 20.34 135 20.87 150 21.62 165 22.40 180 23.20 200 24.49 220 25.81 240 27.09 260 27.37 280 27.35 300 27.34 320 27.31 340 27.31 360 27.27 380 27.25 400 27.24 Give your calculated enthalpy in kJ·mol-1to 3 significant figures

The table below shows the time-temperature course during reaction of NaOH sample of 2.02 g with 169 mL of 1M HCl. Plot the data, evaluate ΔT and calculate the reaction enthalpy. time/s t/ oC 0 19.75 15 19.80 30 19.85 45 19.89 60 19.97 75 20.02 90 19.98 105 20.13 120 20.34 135 20.87 150 21.62 165 22.40 180 23.20 200 24.49 220 25.81 240 27.09 260 27.37 280 27.35 300 27.34 320 27.31 340 27.31 360 27.27 380 27.25 400 27.24 Give your calculated enthalpy in kJ·mol-1to 3 significant figures

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 23Q: Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine...

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Use data from Appendix IIB to calculate ΔS∘rxnΔSrxn∘ for each of the reactions given. 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) Express your answer as an integer. ΔS∘rxn=____________________J/K
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 ethene in the presence of excess oxygen yields carbon dioxide and water: C2H2(g) + 3O2(g) → 2CO2(g) + 2H2O(l) in J/K?
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?
A stoichiometric mixture of CO(g) and H2(g) was allowed to react in two different 2.0L rigid containers at a constant temperature of 298K. The reaction is represented by the equation above. Diagram 1 represents the uncatalyzed reaction and diagram 2 represents the catalyzed reaction one hour after the reactants were mixed. Which of the following correctly explains the experimental results represented in the particle diagrams? A.) Although the reaction is thermodynamically favorable because ΔG°<0 based on the value of K, only the catalyzed reaction could proceed in one hour because its reactant molecules had a higher average kinetic energy. B.) Although the reaction is thermodynamically favorable because ΔG°<0 based on the value of K, only the catalyzed reaction could proceed in one hour because it has a lower activation-energy reaction pathway. C.) The reaction is not thermodynamically favorable because ΔG°>0 based on the value of K, but the addition of a catalyst improved the…
The expression for ∆H° of formation of CO2 as a function of temperature is ∆Ho = -93480–0.603T–0.675x10-4T2-1.091x105/T. Find the ∆Cpo for this reaction as a function of T.
Hess’ Law: ΔH’s of Reaction Steps Add Up to ΔH(tot) [tot] Mg(s) + 1⁄2O2(g) → MgO(s) ΔH(tot) = ___________? [1] Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH1 = _______kJ [2] MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) [3] H2(g) + 1⁄2O2(g) → H2O(l) ΔH2 = _______kJ [3] H2(g) + 1⁄2O2(g) → H2O(l) ΔH3 = –286 kJ
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Urea decomposes in water according to kinetics that are first order in urea. The reaction was found to have a rate constant of 1.2x10^-7 s^-1 at 60 C and 4.6 x10^-7 at 70 C. Calculate the Gibbs energy of activation, the entropy of activation, and the enthalpy of activation for this decomposition (at 60 C). (Show all work please)
You are a chemical engineer working in a pharmaceutical manufacturing plant.You’ve been tasked with scaling up the synthesis of a potential drug candidate.From previous studies, you know the following information about reaction takingplace:ΔHoreaction = -112.2kJΔS = -15.26JK-1mol-1ΔG = -18.81kJ Discuss the meaning of each term/value and what this tells you aboutthe nature of the reaction
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time/s	t/ ^oC
0	19.75
15	19.80
30	19.85
45	19.89
60	19.97
75	20.02
90	19.98
105	20.13
120	20.34
135	20.87
150	21.62
165	22.40
180	23.20
200	24.49
220	25.81
240	27.09
260	27.37
280	27.35
300	27.34
320	27.31
340	27.31
360	27.27
380	27.25
400	27.24