1 of 3 concentrations of NO2 over a period of time in a system that starts out w
ID: 1005716 • Letter: 1
Question
1 of 3 concentrations of NO2 over a period of time in a system that starts out with only NO2. Note Part A - The data table below shows measured that even though the reactants and products are gases, units of measurement are moles per iter (M). Therefore, the notation of brackets are used signifying units of Molarity NeOsl for each measurement. NO, Use stoichiometry to calculate the concentration of N204 at each time. Then, calculate the ratio of (5 reset ?help Measurement # 1 Concentration of I Concentration of [NO/INO.J No 1.00 0.40 0.30 0.15 0.10 0.10 0.00 (Time : 0.00 minutes) 4 7:50 AM 16/2016Explanation / Answer
We know that NO2 and N2O4 can exist in a equilibrium which can be written as
2 NO2 N2O4
a) From this equation its clear that 2 mols of NO2 gives one mol of N2O4 since the table can be written as
[NO2]
[N2O4]
[N2O4]/[NO2]^2
1.00
0.00
---
0.40
0.30
4.44
0.30
0.35
2.448
0.15
0.425
0.830
0.10
0.45
0.4938
0.10
0.45
0.4938
B) For the equilibrium constant values of 0.4938 equilibrium is reached here we can clearly see that neither concentrations of NO2 or N2O4 are changing the equilibrium constant so this condition explains the equilibrium best.
C) Equilibrium constant Kc is given by
Kc = [N2O4]/[NO2]^2
D) The given reaction is reactant favoured because as the reaction progresses the 2 mols of gas will form one mol of gas decreasesing the entropy this leades to a reactant favoured condition.
E) Brown color becomes less intense before stabilising at equilibrium
[NO2]
[N2O4]
[N2O4]/[NO2]^2
1.00
0.00
---
0.40
0.30
4.44
0.30
0.35
2.448
0.15
0.425
0.830
0.10
0.45
0.4938
0.10
0.45
0.4938
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