[A] [B] Rate Experiment 1 1 M 1M

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[A] Rate
Experiment 1 1M 1M 0.1
Experiment 2 1M 3M 0.1
Experiment 3 2M 1M 0.2
2NO(g) + H2(g) à N2O (g) +H2O (g)
In a series of experiments, thefollowing initial rates of disappearance of NO were obtained:
[NO] [H2] rate of loss of NO
Exp. 1 6.4x10-3M 2.2x10-3M 2.6x10-5 M/s
Exp. 2 12.8x10-3M 2.2x10-3M 1.0x10-4 M/s
Exp. 1 6.4x10-3M 4.5x10-3M 5.1x10-5 M/s
Write the rate law and calculate thevalue for the rate constant for the reaction of NO.
CH3CN (g) à CH3CN (g)
The reaction is first order. At 230°Cthe rate constant for the isomerization is 6.3x10-4s-1. What is the half life? How long would it takefor the concentration of CH3CN to decrease to 25% of itsinitial value?
2NO + O2 à 2NO2
The rate law is –D[NO]/Dt =k[NO]2[O2], where k is1.16x10-5 L2/(mol2 s) at339°C. A vessel contains NO and O2 at 339° C. Theinitial partial pressure of NO and O2 are 155 mmHg and345 mmHg respectively. What is the rate of decrease of partialpressure of NO (in mmHg per second)?
Hint from the ideal gas law, obtain anexpression for the molar concentration of a particular gas in termsof its partial pressure. Answer: 6.6x10-8 mmHg/sec
10. Nitryl fluoride is an explosivecompound that is made by the oxidation of nitrogen dioxide withfluorine. 2NO2(g) + F2(g) à 2NO2F(g)
[NO2] mol/L [F2]mol/L [NO2F]mol/L Rate disappearance of NO2 (mol/L*s)
0.0010 0.0050 0.0020 2.0 x 10-4
0.0020 0.0050 0.0020 4.0 x 10-4
0.0020 0.0020 0.0020 1.6 x 10-4
0.0020 0.0020 0.0010 1.6 x 10-4
a. What is the rate law for the reaction?
b. What is the order of the reaction with respect to eachreactant and product?
c. Calculate the rate constant k.
11. Given the following reaction: 2N205 (g) à 2N2O4 (g) +O2 (g)
a. What is the rate constant k for the first order decompositionof N205 (g) at room temperature if thehalf-life at room temperature is 4.03 x 10-4 s?
b. What percentage of N205 (g) moleculeswill NOT have reacted after one day?
12. 2 NO(g) + 2H2 (g) à N2 (g) + 2H2O(g)
For the above reaction, it is observed that when theconcentration of hydrogen gas is cut in half, the rate of thereaction is also cut in half. When the concentration of NO ismultiplied by 10, the rate of the reaction increases by a factor of100.Write the rate expression for this reaction.
13. For the following reaction: 2A + B à C + D
The following results were obtained when the reactionrepresented above was studied at 25 °C
Experiment Initial[A] Initial Initial Rate of Formationof C (mol L-1 min-1)
1 0.25 0.75 4.3 x 10 -4
2 0.75 0.75 1.3 x 10 -3
3 1.50 1.50 5.3 x 10 -3
4 1.75 ?? 8.0 x 10-3
a) Determine the order of the reaction with respect to A and B.Justify your answer.
b) Write the rate law for the reaction. Calculate the value ofthe rate constant, specifying units.
c) Determine the initial rate of change of [A] in Experiment3.
d) Determine the initial value of in Experiment 4.