Answered: Given the AH°f and S° values below,…

Given the AH°f and S° values below, what is the boiling point of Br2? So AH°f (kJ/mol) (J/ mol K) Br2(1) -239 127 Br2(8) -201 240 O 273 K 336 K 373 K 1199 K O 2.1 K

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...

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Based on the thermodynamic properties provided for methanol (below), select from the following list the equation(s) necessary to calculate the amount of energy needed for 5.0 kg of methanol to go from -64°C to 88°C. Property Value Units Melting point -94 °C Boiling point 65 °C AHfus 3.18 kJ/mol AHvap 37 kJ/mol 615) 48.7 J/mol.°C Cp (1) 81.1 J/mol.°C 5 (8) 43.8 J/mol °C Choose one or more: A. q = n(43.8 J/mol °C)AT, where AT is negative B. q=n(48.7 J/mol ·°C)AT, where AT is negative C. q= n(81.1 J/mol -°C)AT, where A Tis negative D. q = n(43.8 J/mol °C)AT, where A Tis positive E. q=n(-3.18 kJ/mol) F. q- n(37 kJ/mol) G. q=n(-37 kJ/mol) H. q- n(3.18 kJ/mol) 1.q=n(48.7 J/mol °C)AT, where AT is positive J.q=n(81.1 J/mol °C)AT, where A Tis positive
How many kilojoules (kJ) of energy would be required to raise the temperature of 200.0 grams of water from 25.00 °C to 100.0 °C? csp of water is 4.184 J g-1 °C-1
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53. What mass of water initially at -12.5 °C can be converted to liquid water at 27.9 °C by 38.36 kJ of energy? AHfus = 334 J/g AHvap =2261 J/g Csolid=2.11 J/g.°C Cliquid 4.18 J/g °C Cgas = 2.01 J/g °C A. 80.4 g B. 91.5 g C. 76.3 g D. 268 g =
I am confused by only K value. I think it is Substituting the values: ln(K) = -(-3.9 × 105 J/mol) / (8.314 J/K.mol × 298 K) = 157.41 Taking the exponential of both sides gives: K = e^157.41 K = 2.3 X 10^68
1. Calculate the AS (J/K) for the phase transition of a 0.50 mol water described below: H2O(s), 0°C → H2O(g), 100°C Afus H = 60 kJ/mol, C'p,H,0, = 75.3 J/mol-K, Apap H = 40.7 kJ/mol
Methane-producing bacteria convert liquid acetic acid (CH3CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHOrxn = kJ Calculate AG rxp = (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)
From this reaction 2NO(g) + 2H₂(g) à N₂(g) + 2H₂O(1), NO H2 N2 Sᵒ (J/mol K) 75.10 191.5 192.3 ΔΗ°f (kJ/mol) -283.74 0 0 What is the standard enthalpy of reaction (AHrnx)? H20 189.0 -373.57
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Using the following thermochemical data: 2Er(s) + 6HF(g) → 2ErF3(s) + 3H2(g) ΔH° = -1795.4 kJ/mol 2Er(s) + 6HCl(g) → 2ErCl3(s) + 3H2(g) ΔH° = -1443.6 kJ/mol calculate ΔH° for the following reaction:ErF3(s) + 3HCl(g) → ErCl3(s) + 3HF(g) 351.8 kJ/mol -3239.0 kJ/mol -1619.5 kJ/mol 703.6 kJ/mol 175.9 kJ/mol
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