Calculate the degree of dissociation of N2O4 in the reaction : N2O4(g) → 2NO2(g) at 250 K and a total pressure of 0.500 bar. Do you expect the degree of dissociation to increase or decrease as the temperature is increased to 550 K? AG?(NO2,g)= 51.3x10³ J /mol, AGf'(N2O4,g)= 99.8x10° J /mol at 25°C AHF (NO2,g)= 33.2x10° J /mol, AH£°(N204,g)= 11.1x10° J /mol at 25°C %3D

Calculate the degree of dissociation of N2O4 in the reaction : N2O4(g) → 2NO2(g) at 250 K and a total pressure of 0.500 bar. Do you expect the degree of dissociation to increase or decrease as the temperature is increased to 550 K? AG?(NO2,g)= 51.3x10³ J /mol, AGf'(N2O4,g)= 99.8x10° J /mol at 25°C AHF (NO2,g)= 33.2x10° J /mol, AH£°(N204,g)= 11.1x10° J /mol at 25°C %3D

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 51E: In the laboratory, hydrogen chloride (HCl(g)) and ammonia (NH3(g)) often escape from bottles of...

See similar textbooks

Similar questions

In the laboratory, hydrogen chloride (HCl(g)) and ammonia (NH3(g)) often escape from bottles of their solutions and react to form the ammonium chloride (NH4Cl(s)), the white glaze often seen on glassware. Assuming that the number of moles of each gas that escapes into the room is the same, what is the maximum partial pressure of HCl and NH3 in the laboratory at room temperature? (Hint: The partial pressures will be equal and are at their maximum value when at equilibrium.)
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.
The value of Delta G at 261.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) +3Cl2 (g) -> 2PCI3 (g) is ___ kJ/mol. at 25.0oC for this reaction, delta H is -720.kJ/mol, Delta G is -642.9kJ/mol and delta s is -263.7 J/K
10. What is ∆G for the decomposition of CaCO3 at 298K and a partial pressure of CO2 of 4*10-4 bar? ∆Gf0 for CaCO3(s), CaO(s) and CO2(g) are -1129 kJ/mol, -604 kJ/mol and -394 kJ/mol, respectively. CaCO3(s) → CaO(s) + CO2(g) A. 0 B. -131 kJ/mol C. 112 kJ/mol D. 131 kJ/mol E. 150 kJ/mol (Correct answer is C, I'm just looking for an explanation!).
Sucrose enters a series of reactions in glycolysis after the reaction in which it is hydrolyzed, forming glucose and fructose: The quotient, Q, value for this reaction = 5.3 × 1012 at 298 K. What is the value of ΔGorxn?
For the reaction A (g) → 2 B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298 K when ∆G = -19.3 kJ/mol?
Calculate the degree of decomposition of n2O4 to NO2(g) at 0.49 bar total pressure and 300K. If the temperature increases to 600C, how does the degree of decomposition change (increase-decrease) and why?
At 25 ∘C25 ∘C, the equilibrium partial pressures for the reaction 3A(g)+3B(g)↽−−⇀C(g)+3D(g)3A(g)+3B(g)↽−−⇀C(g)+3D(g) were found to be ?A=4.38PA=4.38 atm, ?B=4.26PB=4.26 atm, ?C=4.32PC=4.32 atm, and ?D=4.83PD=4.83 atm. What is the standard change in Gibbs free energy of this reaction at 25 ∘C25 ∘C?
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) A )Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc = _____/_____ = _____ Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the concentration of O₂ at equilibrium. [O₂]eq = _____M
The dissociation of N2O4(g) is important in photochemical air pollution, like that common in Los Angeles, California. The reaction can be written N2O4(?) ⇆ 2NO2(?) Will the fraction of molecules dissociated increase or decrease when the temperature is raised to 555 K? Assume that ΔrH is independent of temperature.
For the following reaction: X(g) ⇌ 2Y(g) + Z(g) The value of ΔH° is -219 kJ/mol, and that of ΔG° is -372 kJ/mol · K. Determine ΔS° in J/mol at 25°C.