H_{2}O_{2} decomposes at 20˚C in a first order reaction where k = 1.06 x 10^{3}min^{1}. If the initial concentration of H_{2}O_{2} is 0.020 M, what is [H_{2}O_{2}] after 3.5 days?
a. 
9.6x10^{5} M 

b. 
5.1x10^{5} M 

c. 
4.4x10^{5} M 

d. 
1.7x10^{5} M 
For the following reaction, calculate the average reaction rate over the last 2 minutes using the table of data below.
H_{2(g)} + 2ICl_{(g)} I_{2(g)} + 2HCl_{(g)}
Time (min) [ICl] (M)
 
0 2.000
2 1.052
4 0.748
6 0.586
a. 
0.0900 M/min 

b. 
0.175 M/min 

c. 
0.0405 M/min 

d. 
0.352 M/min 
Which statement(s) below do we know is (are) true about the following net reaction?
2N_{2}O_{5} 2N_{2} + 5O_{2}
a. 
The rate law = k[N_{2}O_{5}]^{2} 

b. 
The reaction rate = 1/2(∆[N_{2}]/∆t) 

c. 
The reaction rate = 1/2(∆[N_{2}O_{5}]/∆t) 

d. 
The reaction rate = 1/5(∆[O_{2}]/∆t) 

e. 
a & b 

f. 
b & c 

g. 
c & d 

h. 
a, b, & c 

i. 
b, c, & d 

j. 
All are true 
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