What is the half-life of a first-order reaction if the rate constant is 6.2 x 10-3 s-1?
The elementary steps for the catalyzed decomposition of dinitrogen monoxide are shown below.
N2O(g) + NO(g) ® N2(g) + NO2(g)
NO2(g) ® NO(g) + 1/2 O2(g)
Which of the following statements is/are CORRECT?
|
1.
|
The overall balanced reaction is N2O(g) ® N2(g) + 1/2 O2(g).
|
|
2.
|
NO2(g) is a catalyst for the reaction.
|
|
3.
|
NO(g) is a reaction intermediate.
|
Given the initial rate data for nitrogen monoxide and oxygen reaction,
2 NO(g) + O2(g) ® 2 NO2 (g)
was measured at 25 C for various concentrations of NO and O2. Determine the rate equations from these data.
|
Experiment
|
Conc [NO] (mol/L)
|
Cone [O2] (mol/L)
|
Initial Rate (mol/L s)
|
|
1
|
0.020
|
0.010
|
0.028
|
|
2
|
0.020
|
0.020
|
0.057
|
|
3
|
0.020
|
0.040
|
0.114
|
|
4
|
0.040
|
0.020
|
0.227
|
|
5
|
0.010
|
0.020
|
0.014
|
Which statement concerning relative rates of reaction is correct for the decomposition of phosphine?
4 PH3(g) → P4(g) + 6 H2(g)
A. The rate of disappearance of PH3 is 6/4 the rate of appearance of H2
B. The rate of appearance of P4 is equal to the rate of appearance of H2.
C. The rate of disappearance of PH3 is 1/4 the rate of appearance of P4.
D. The rate of disappearance of PH3 is 1/4 times the rate of appearance of H2.
E. The rate of appearance of H2 is 1/6 times the rate of appearance of P4