Question

The following data was collected for the reaction of ammonium ion and nitrite ion: Reaction data...

The following data was collected for the reaction of ammonium ion and nitrite ion:
Reaction data for the reaction of ammonium and nitrite ions in water at 25 oC
NH4+(aq) + NO2-(aq) --> N2(g) + 2H2O(l)

Experiment Number Initial Concentrations (M) Initial Concentrations (M) Observed Initial Rate of Reaction (M s-1​)
NH4​+ NO2-
1 0.0100 0.200 5.4 x 10-7
2 0.0200 0.200 10.8 x 10-7
3 0.0400 0.200 21.5 x 10-7
4 0.0600 0.200 32.3 x 10-7
5 0.200 0.0202 10.8 x 10-7
6 0.200 0.0404 21.6 x 10​-7
7 0.200 0.0606 32.4 x 10-7
8 0.200 0.0808 43.3 x 10-7

a) What is the rate law for this reaction? i) Rate = k[NH4+][NO2-], ii) Rate = k[NH4+]2[NO2-], iii) Rate = k[NH4+][NO2-]2​, iv) Rate = k[NH4+][NO2-]0
​b) What is the rate constant?​ i) 5.40 x 10-7 s M-1, ii) 3.23 x 10-6 s M-1, iii) 2.68 x 10-4 s M-1, iv) 7.63 x 10-3 s M-1
​c) If the initial concentrations of NH4+ and NO2- are 0.300 and 0.500 M respectively at the beginning of an experiment, what is the concentration of NH4+ after 2 hours? i) 0.137 M​, ii) 0.169 M, iii) 0.363 M, iv) 0.467 M

Homework Answers

Answer #1


order w.r.t NH4+

r1/r2 = (a1/a2)^x

((5.4*10-7)/(10.8*10^-7)) = (0.01/0.02)^x

x = 1

order w.r.t NO2-


r5/r6 = (a5/a6)^y

((10.8*10^-7)/(21.6*10^-7)) = (0.0202/0.0404)^y


y = 1

over all order = 1+1 = 2

a) rate law , rate = k[NH4+[NO2-]

Answer: i

b) rate constant(k) = rate / [NH4+[NO2-]

                   = 43.3*10^-7/(0.2*0.808)

                   = 2.68*10^-5 M-1.S-1

answer: iii

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The following initial rate data are for the reaction of ammonium ion with nitrite ion in...
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+ + NO2- N2 + 2 H2O Experiment [NH4+]o, M [NO2-]o, M Initial Rate, Ms-1 1. 0.296 0.180 1.85×10-5 2. 0.296 0.361 3.72×10-5 3. 0.592 0.180 3.71×10-5 4. 0.592 0.361 7.44×10-5 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power...
The reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2- --->   N2...
The reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2- --->   N2 + 2 H2O is first order in NH4+ and first order in NO2-. Complete the rate law for this reaction. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to...
Consider the reaction of ammonium ions (NH4+) and nitrite ions (NO2-) shown in equation below:      ...
Consider the reaction of ammonium ions (NH4+) and nitrite ions (NO2-) shown in equation below:                   NH4+ (aq) + NO2-(aq) → N2(g) + 2 H2O(l) Determination Number Initial [NH4+], M Initial [NO2-], M Initial rate, Ms-1 1 0.15 0.0075 3.0 x 10-7 2 0.15 0.015 6.0 x 10-7 3 0.30 0.015 1.2 x 10-6 (a) Use method of initial rates to find the order of the reaction with respect to NH4+. (b) Use the method of initial rates to...
For the reaction between the peroxydisulfate ion (S2O82-) and the iodide ion in aqueous solution: S2O82-...
For the reaction between the peroxydisulfate ion (S2O82-) and the iodide ion in aqueous solution: S2O82- (aq) + 3I- (aq) → 2SO42- (aq) + I3- (aq) An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. What is the average rate of disappearance of I- in the initial 400.0 s, between 400.0 s and 800.0...
Anila performed the following reactions between oxalic acid (H2C2O4) and Permanganate ion and measured the reaction...
Anila performed the following reactions between oxalic acid (H2C2O4) and Permanganate ion and measured the reaction time at a constant temperature: MnO4-(aq) + H2C2O4(aq) --> MnO2(aq) + CO2(g) + (other products) rate = k[MnO4-]x [H2C2O4]y Determination Initial [MnO4-], mol/L Initial [H2C2O4], mol/L Elapsed time (Δt), s Reaction rate, mol/L·s 1 0.0230 0.120 224 2 0.0230 0.240 111 3 0.0460 0.240 110 a) (3 pts) Calculate the reaction rate of the determination 2, using reaction rate = -Δ[MnO4-]/Δt. b) (3 pts)...
Consider the following reaction between mercury(II) chloride and oxalate ion: 2HgCl2(aq)+C2O2−4(aq)→2Cl−(aq)+2CO2(g)+Hg2Cl2(s) The initial rate of this...
Consider the following reaction between mercury(II) chloride and oxalate ion: 2HgCl2(aq)+C2O2−4(aq)→2Cl−(aq)+2CO2(g)+Hg2Cl2(s) The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O2−4, and the following rate data were obtained for the rate of disappearance of C2O2−4: Experiment HgCl2(M) C2O2−4(M) Rate (M/s) 1 0.164 0.15 3.2×10−5 2 0.164 0.45 2.9×10−4 3 0.082 0.45 1.4×10−4 4 0.246 0.15 4.8×10−5 1. What is the reaction rate when the concentration of HgCl2 is 0.110 M and that of C2O2−4 is...
The following data were obtained at 25C for a reaction: aA + bB = cC Initial...
The following data were obtained at 25C for a reaction: aA + bB = cC Initial Concentrations Initial Reaction Rate Reaction [A] [B] M/s or mol/Ls 1 0.100 M 0.200 M 5.00x10^-4 2 0.150 M 0.200 M 7.50x10^-4 3 0.150 M 0.600 M 6.75x10^-3 What is the order of the reaction with respect to A? What is the order of the reaction with respect to B? What is the rate constant, k, for the reaction?
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) U4+ (aq) →...
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) U4+ (aq) → UO22+ (aq) (ii) (acid solution) Rh2+ (aq) → Rh2O3 (s) (iii) (base solution) MnO2 (s) → MnO4– (aq) (iv) (base solution) PuO3 (s) → Pu(OH)4 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations...
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial Rate (M/s) 0.15 6.87×10−3 0.30 1.37×10−2 0.60 2.75×10−2 What is the rate law for this reaction? Rate = k[A]3 Rate = k[A] Rate = k Rate = k[A]2 2.) Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial Rate (M/s) 0.15 2.75×10−2 0.30 2.75×10−2 0.60 2.75×10−2 What is the...
Determine the rate law and the value of k for the following reaction using the data...
Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4 0.084 4.37 x 10-4 0.224 1.16 x 10-3 Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4 0.084 4.37 x 10-4...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT