If we have a initial concentration of H4NO2 (aq) at .10 M, make an ICE table...
If we have a initial concentration of H4NO2 (aq) at .10 M, make an ICE table for the following reaction, and solve for the concentration of NH4, NO2, NH3 and HNO2
NH4+(aq)+NO2-(aq)<=>NH3(aq)+HNO2(aq)
(not sure if this helps, but the value of K1 is 1.23e-6)
Homework Answers
![-4 . [NH₂] = [HNO2) = x= 1.89 x 10 9 (M) [NHst] = [NO] = 0.1-4 = 0.09989 (M)](http://img.homeworklib.com/questions/6196e790-d9dc-11eb-b3ec-85e4058692a1.png?x-oss-process=image/resize,w_560)
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If we have a initial concentration of
H4NO2 (aq) at .10 M, make an ICE table...
PART A is already solved. It is provided for context for you :) PART A: If...
PART A is already solved. It is provided for context for you :) PART A: If you have a initial conc. 0.10M NH4NO2, make an ICE table, solve for concentration of NH4+, NO2-, NH3 and HNO2.K1 value is 1.23e-6 NH4+NO2<=>NH3+HNO2 [NH4] and [NO2] both are 9.99e-2 M [NH3] and [HNO2] were found to be 1.11e^-4 M PART B (the part I need help with): Using the values you found in part A (conc. of NH4 and NH3), find the value...
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2...
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2 k1? NH4+ + H2O -> H3O+ + NH3. ka = 5.6 x 10^-10 NO2- + H2O -> HNO2 + OH- kb =2.2 x 10^-11 2H2O -> H3O+ + OH- kw = 1.0 x10^-14 Write symbolic expression for equilibrium constants for each reaction. Derive expression for k1 in terms of ka, kb, and kw; find numerical value of k1.
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq)...
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Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (N...
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Initial rate data are listed in the table for the reaction: Initial rate data are listed...
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Initial rate data are listed in the table for the
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First determine the rate law and rate constant.
Under the same initial conditions as in Experiment
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The units should be M, and should be calculated to
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Initial rate data are listed in the table for the reaction:
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2 (g) + H20 (1) Experiment (NH4+]: [NO 2-1. Initial rate (M/s) 0.24 0.10 7.2 x 10-4 0.10 3.6 x 10-4 10.12 0.15 5.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+] at...
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First determine the rate law and rate constant.
Under the same initial conditions as in Experiment
4, calculate [NH4+] at 184 seconds after
the start of the reaction. In this experiment, both reactants are
present at the same initial concentration.
The units should be M, and should be calculated to
three significant figures.
1:26 Bb Bb # ....
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