For a particular reaction, AH° = 55.4 kJ/mol and AS° = 94.1 J/(mol-K). Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? %3D %3D T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? greater than less than

For a particular reaction, AH° = 55.4 kJ/mol and AS° = 94.1 J/(mol-K). Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? %3D %3D T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? greater than less than

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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For a particular reaction, AH° = -93.8 kJ and AS° = –156.1 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.
From the values of ΔH and ΔS calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -389 kJ/mol, ΔS = 27.8 J/K · mol
For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?
Consider the reaction below for the decomposition of carbon tetrachloride gas: CCl4(g) ------> C(s) + 2Cl2 (g) ΔH = + 95.7 kJ; ΔS = + 142.2 J/K If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.
The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol
A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous? 626.4 K This reaction is always spontaneous 498.3 K 434.6 K This reaction is never spontaneous
For a given reaction, ΔH∘∘= +35.5 kJ/mol and ΔS∘∘= +83.6 J/(K∙∙ mol). In what temperature range is the reaction spontaneous? Assume that ΔH∘∘ and ΔS∘∘ do not vary with temperature.
Consider the following reaction: CaCO 3(s) <—> CaO (g) +CO 2(g) For this reaction, delta S = +158.9 J/ mol and Delta * H ^ o = + 177.9kJ / (mol) . These values are fairly constant with changes in temperature. Over what specific temperature range is this reaction spontaneous in the forward direction?
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Which are spontaneous at all temperatures? Choose one or more: 2H,0(g) + SO,(g) - 152.4 J/K 2H,S(g) +30,(g) AH°. rxn = - 1037 kJ, AS°. rxn → 2SO3(g) - 197.8 kJ, ASº. 2SO,(g) +O2(g) AH°. rxn - 187.8 J/K rxn O so,(8) + H,0(1) → H,SO4(1) AH°. rxn - 132.5 kJ, AS° - 169.9 J/K rxn S(g) +O2(8) –→ SO,(g) - 574.0 kJ, AS°, ΔΗ. rxn - 124.6 J/K rxn none of the above