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Document Preview: The data in the table below were obtained for the reaction:What is the order of the reaction with respect to?       A) 1 B) 0 C) 2 D) 3 E) 4  What is the order of the reaction with respect to ? A) 0 B) 1       C) 2       D) 3      E) 4 The reaction follows second-order kinetics. At 300 °C, drops from XXXXXXXXXXM to XXXXXXXXXXM in 100.0 s. The rate constant for the reaction is __________. A) 0.096 B) 0.65 C) 0.81 D) 1.2 E) 0.5419) A compound decomposes by a first-order process. If  of the compound decomposes in 60.0 minutes, the half-life of the compound is _________. A) 65 minutes B) 120 minutes C) 145 minutes D) 180 minutes E) 198 minutesThe reaction  is first order in [A]. Consider the following data. 5) The rate constant for this reaction is __________. A) 0.013 B) 0.030 C) 0.14 D) 3.0 E) 6) The reaction  is first order in [A].  A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds:The rate constant for this reaction is __________.  A) 0.23 B) 1.0 C) 0.17 D) 0.12 E) 7) At elevated temperatures, methylisonitrile isomerizes to acetonitrile:       CH3NC (g XXXXXXXXXXCH3CN (g)The dependence of the rate constant on temperature is studied and the graph below is prepared from the results.  The energy of activation of this reaction is __________ kJ/mol. A) 160 B) C) D) E) 8) For the elementary reaction The molecularity of the reaction is __________, and the rate law is A) 2, B) 4, C) 2, D) 2, E) 4,9) A particular first-order reaction has a rate constant of at. What is the magnitude of k at  if A) B) C) 576 D) E) 10) For a certain chemical reaction, the rate constant triples (K2= 3K1 ) as the temperature increases from 15oC to 25oC. Calculate the activation energy (Ea). 78400 kJ/mol8.2 J/mol7.84 kJ/mol8200 kJ/mol0.86 J/mol11) What would be the effect of decreasing the pressure by increasing the volume on the following system at...

David · Accepted Answer

1
 
1. The data in the table below were obtained for the reaction: 
 
2 3 2 22ClO (aq) 2OH (aq) ClO (aq) ClO (aq) H O(l)
     
What is the order of the reaction with respect to 2ClO ?  
      A) 1  
B) 0  
C) 2  
D) 3  
E) 4   
Explanation – 0.0248/0.00276 = (0.060/0.020)^a * (0.03/0.03)^b 
9 = (3^a) * (1^b) 
Since 1 to the 
Thus a = 2
2. What is the order of the reaction with respect to OH ?  
 
A) 0  
B) 1  
      C) 2  
      D) 3 
      E) 4
Explanation - 0.00276/0.00828 = (0.030/0.090)^b 
1/3 = (1/3)^b 
Thus, b=1
3. The reaction follows second-order kinetics. At 300 °C, 2[NO ] drops from 0.0100 M to 
0.00650 M in 100.0 s. The rate constant for the reaction is __________ 1 1M s  . 
2 2 2NO 2NO O    
A) 0.096  
B) 0.65  
C) 0.81  
D) 1.2  
E) 0.54
Ans. [NO2]final = 1/ ((1/[NO2]initial) + kt) 
0.00650 = 1/ ((1/0.0100) + k(100)) 
0.00650 = 1/ (100+ 100k) 
100+ 100k = 1/0.00650 
100 + 100k = 153.8 
K = 53.8/100 = 0.54
4. 19) A compound decomposes by a first-order process. If 25.0 %  of the compound 
decomposes in 60.0 minutes, the half-life of the compound is _________.  
A) 65 minutes  
B) 120 minutes  
C) 145 minutes  
D) 180 minutes  
E) 198 minutes
Ans. The concentration-time equation for a first order reaction is
ln ([A]t / [A]o) = -kt . . .where ([A]t / [A]o) is the fraction of reactant remaining (75.0% = 
0.750).
ln (0.750) = -(k)(60.0 min) 
-0.288 = -(k)(60.0 min) 
k = 0.00479 min^-1
The half-life for a first order reaction is
t1/2 = 0.693 / k = 0.693 / 0.00479 min^-1 = 145 min^-1
5.) The reaction A  B  is first order in [A]. Consider the following data. 
 
 
 The rate constant for this reaction is __________ 1s .
A) 0.013  
B) 0.030  
C) 0.14  
D) 3.0  
E) 33.1 10  
Explanation- from the data it can be seen that t1/2 of the reaction is 5s 
Thus k = 0.693/5 = 0.14s-1
6) The reaction A(aq) B(aq)  is first order in [A].

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