The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored...
The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ∘C we have the following values for the standard state enthalpy and free energy changes of the reaction: ΔH∘=+109.6kJ/mol ΔG∘=−30.5kJ/mol c. What is driving the reaction forwards: enthalpy, entropy or both?
Homework Answers
It is both the enthalpy and entropy of the reaction which drives the reaction in forward direction as if we substitute the values in formaula delta G= detla H -T delta S , we get Delta S= 470KJ/ K/mol and delta H = 109.6 KJ/ mol. Since both are positive so the reaction is in forward direction .
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The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is
an example of a reaction that is thermodynamically favored...
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is...
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state entrapped and free energy changes of the reaction: ΔH° = +109.6 kJ/mol ΔG° = -30.5 kJ/mol a. Calculate ΔS° at 25°C b. Why is the entropy change so favorable for this reaction? Please answer and explain both questions!
Need the answer to part B The decomposition of crystalline N, O N,Og(s) + 2NO2(g) +...
Need the answer to part B
The decomposition of crystalline N, O N,Og(s) + 2NO2(g) + 0(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state enthalpy and free energy changes of the reaction: AH = +109.6 kJ/mol AG° = -30.5 kJ/mol Part A Calculate AS at 25°C. Express your answer with the appropriate units. AS° = 470 melk Submit Previous Answers All...
The first-order rate constant for the decomposition of N2O5, N2O5(g) 2NO2(g) + O2(g)At 70C is 6.810-3s-1....
The first-order rate constant for the decomposition of N2O5, N2O5(g) 2NO2(g) + O2(g)At 70C is 6.810-3s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 1.0 L. a.) How many moles of N2O5will remain after 2.5 min? b.)How many minutes will it take for the quantity of N2O5to drop to 0.010 mol? c.What is the half-life of N2O5at 70 degrees C?
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form...
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes...
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
Calculate the Entropy of the reaction equilibrium between 2NO2 - N2O4 given the equation: Delta G...
Calculate the Entropy of the reaction equilibrium between 2NO2 - N2O4 given the equation: Delta G = Delta H - T Delta S where: Enthalpy = -47.5 Kj/mol Gibbs free energy = -3.59 Kj/mol Temperature = 298K
Calculate the changes in free energy, enthalpy, and entropy when 1.00 mol Ar(g) at 27°C is...
Calculate the changes in free energy, enthalpy, and entropy when 1.00 mol Ar(g) at 27°C is compressed isothermally from 100.0 L to 15.0 L. ΔH = _____kJ ΔS = _____J/K ΔG = _____kJ
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330...
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330°C the rate constant for the decomposition of NO2 is 0.775 L/(mol sec) Suppose the initi concentration is 0.0030 mol/L. What is the concentration of NO2 after 645 s?
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of...
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of N2O4 became 2 times less after 2,5⋅103 s. You have to calculate: a) the value of rate constant k of the reaction; b) the value of equilibrium constant Kp. You are given the value of standard Gibb’s energy of formation Goform: substance Goform, kJ/mol NO2(g) 51.6 N2O4(g) 98.4
6. The following reaction shows decomposition of ammonium hydrosulfide. NH4SH(s) ↔ NH3(g) + H2S(g) ; Kc...
6. The following reaction shows decomposition of ammonium hydrosulfide. NH4SH(s) ↔ NH3(g) + H2S(g) ; Kc = 1.2 x 10-4 at 25 ºC a) Calculate standard Gibbs free energy (∆Gº) for this reaction. Is this reaction spontaneous? b) If ΔSº of this reaction is 281.2 J/K∙mol, calculate enthalpy of this reaction. Is this reaction exothermic or endothermic?
Need the answer to part B
The decomposition of crystalline N, O N,Og(s) + 2NO2(g) + 0(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state enthalpy and free energy changes of the reaction: AH = +109.6 kJ/mol AG° = -30.5 kJ/mol Part A Calculate AS at 25°C. Express your answer with the appropriate units. AS° = 470 melk Submit Previous Answers All...
Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330°C the rate constant for the decomposition of NO2 is 0.775 L/(mol sec) Suppose the initi concentration is 0.0030 mol/L. What is the concentration of NO2 after 645 s?
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