Consider this reaction occurring at 298 K: N 2 O ( g ) + NO 2 ( g ) ⇌ 3 NO ( g ) Show that the reaction is not spontaneous under standard conditions by calculating Δ G rxn ° . If a reaction mixture contains only N 2 O and NO 2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
Consider this reaction occurring at 298 K: N 2 O ( g ) + NO 2 ( g ) ⇌ 3 NO ( g ) Show that the reaction is not spontaneous under standard conditions by calculating Δ G rxn ° . If a reaction mixture contains only N 2 O and NO 2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
Solution Summary: The author explains that the reaction N 2 O + N O 2 is not spontaneous under standard conditions. The enthalpy of spontaneity can be determined using the change in Gibbs free energy.
Show that the reaction is not spontaneous under standard conditions by calculating
Δ
G
rxn
°
.
If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?
Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
(c) The following data have been obtained for the hydrolysis of sucrose, C12H22O11, to
glucose, C6H12O6, and fructose C6H12O6, in acidic solution:
C12H22O11 + H2O → C6H12O6 + C6H12O6
[sucrose]/mol dm³
t/min
0
0.316
14
0.300
39
0.274
60
0.256
80
0.238
110
0.211
(i) Graphically prove the order of the reaction and determine the rate constant of the
reaction.
(ii) Determine the half-life, t½ for the hydrolysis of sucrose.
(III) adsorbent
(b) Adsorption of the hexacyanoferrate (III) ion, [Fe(CN)6] ³, on y-Al2O3 from aqueous
solution was examined. The adsorption was modelled using a modified Langmuir
isotherm, yielding the following values of Kat pH = 6.5:
(ii)
T/K
10-10 K
280
2.505
295
1.819
310
1.364
325
1.050
Determine the enthalpy of adsorption, AadsHⓇ.
If the reported value of entropy of adsorption, Aads Se = 146 J K-1 mol-1 under the above
conditions, determine Aads Gº.
with full details solution please
Chapter 18 Solutions
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