4. Consider the reaction of ammonium ions (NH*) and nitrite ions (NO,"), shown in Equation 19. NH,*(aq) + NO," (aq) → N2(g) + 2 H20(!) (Eq. 19) Solutions containing NH,* and NO, were mixed in various quantities and the following rate data at a constant temperature were obtained: initial NO2 initial rate for initial NH concentration, determination concentration, formation of N2 number moVL mo/L mol/L's 7.50 × 10-3 1.50 x 10-2 1.50 x 10-2 3.04 x 10-7 6.08 x 10-7 1.22 x 10-6 0.150 0.150 0.300 (c) Calculate the rate constant, k, for the reaction of NH,* and NO,. (a) Use the method of initial rates to find the or- der of the reaction with respect to NH. (b) Use the method of initial rates to find the order of the reaction with respect to NO2. (d) Write the rate equation for the reaction of NH, and NO,.

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72
KINE 505: Studying the Rate of Reaction of Potassium Permanganate and Oxalic Acid
4. Consider the reaction of ammonium ions (NH+) and nitrite ions (NO,), shown in Equation 19.
NH,(aq) + NO, (aq) → N2(g) + 2 H20(1)
(Eq. 19)
Solutions containing NH and NO, were mixed in various quantities and the following rate data at a constant
temperature were obtained:
initial NH
concentration,
initial NO2
initial rate for
determination
concentration,
formation of N2
b
number
mol/L
mol/L
mol/L's
7.50 x 10-3
1.50 x 10-2
1.50 x 10-2
3.04 x 10-7
6.08 x 10-7
1.22 x 10-6
1
0.150
0.150
ap
3
0.300
(a) Use the method of initial rates to find the or-
der of the reaction with respect to NH*.
(c) Calculate the rate constant, k, for the reaction
of NH,* and NO2.
shi
(d) Write the rate equation for the reaction of
NH,* and NO,.
Use the method of initial rates to find the order
(b)
of the reaction with respect to NO2.
Transcribed Image Text:72 KINE 505: Studying the Rate of Reaction of Potassium Permanganate and Oxalic Acid 4. Consider the reaction of ammonium ions (NH+) and nitrite ions (NO,), shown in Equation 19. NH,(aq) + NO, (aq) → N2(g) + 2 H20(1) (Eq. 19) Solutions containing NH and NO, were mixed in various quantities and the following rate data at a constant temperature were obtained: initial NH concentration, initial NO2 initial rate for determination concentration, formation of N2 b number mol/L mol/L mol/L's 7.50 x 10-3 1.50 x 10-2 1.50 x 10-2 3.04 x 10-7 6.08 x 10-7 1.22 x 10-6 1 0.150 0.150 ap 3 0.300 (a) Use the method of initial rates to find the or- der of the reaction with respect to NH*. (c) Calculate the rate constant, k, for the reaction of NH,* and NO2. shi (d) Write the rate equation for the reaction of NH,* and NO,. Use the method of initial rates to find the order (b) of the reaction with respect to NO2.
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