The rate law
The N2O decomposition reaction is represented by the following equation:
2 N2O(g) → 2 N2(g) + O2(g)
This reaction is first order, and k = 3.40 s-1 at a certain temperature.
In an experiment at the same temperature, the initial concentration of N2O is 0.27 M. Determine how many seconds for the initial 50% decomposition of N2O: t =____ second
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The decomposition of nitrous oxide at 565 °C N2O(g)----> N2(g) + ½ O2(g) is second order...
The decomposition of nitrous oxide at 565 °C N2O(g)----> N2(g) + ½ O2(g) is second order in N2O. In one experiment, when the initial concentration of N2O was 0.790 M, the concentration of N2O dropped to 0.103 M after 5.21×10^3 seconds had passed. Based on these data, the rate constant for the reaction is _____________ M-1 s-1.
1A. The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N2O5 2 NO2...
1A. The decomposition of dinitrogen pentoxide in carbon
tetrachloride solution at 30 °C N2O5 2 NO2 + ½ O2 is first order in
N2O5 with a rate constant of 4.10×10-3 min-1. If the initial
concentration of N2O5 is 0.510 M, the concentration of N2O5 will be
M after 402 min h
1B. The gas phase decomposition of phosphine at 120 °C
PH3(g)1/4
P4(g) + 3/2 H2(g)
is first order in PH3
with a rate constant of 1.80×10-2
s-1.
If the...
Question #: 13 The metal-catalyzed decomposition of N2O was studied to determine the overall order of...
Question #: 13 The metal-catalyzed decomposition of N2O was studied to determine the overall order of the reaction. 2 N2O(g) +2 N2(g) + O2(g) As the reaction of N20 was monitored, half of the N20 reacted at 15 seconds, and all the remaining N20 reacted in the next 15 seconds. What is the order of the reaction? A. zeroth-order B. first-order C. second-order D. third-order
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g)...
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second order with respect to NO(g) and first order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.6 x 102 M–2 s–1. When the initial concentrations of NO and O2 are 0.02 M and 0.015 M, respectively, the rate of the reaction is ___ M/s. 1b. The rate constant of a first-order decomposition reaction is 0.014...
1.) The reaction A (aq)-->B (aq) is a first order reaction where the haf life of...
1.) The reaction A (aq)-->B (aq) is a first order reaction where the haf life of A (aq) of the reaction at 25 degrees celsius is 377 seconds. The half life of the reaction at 35 degrees celsius is 333 s. What is the necessary time for the concentration of A (aq) to fall from 0.777 M to 0.222 M at 50 degrees celsius? The answer is 507 seconds? 2.) THe N2O (g) decomposes to give N2 (g) and O2...
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) +...
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) + N2O(g) --> N2(g) + NO2(g) (slow) 2 NO2(g) --> 2 NO(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [N2O]2 Rate = k [NO] [NO2] Rate = k [N2O]2 [N2O] Rate = k [NO2] [N2O] Rate = k [N2O] [N2O] Rate = k [NO] [N2O] (b) Choose...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial ra...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
The decomposition of NO2 at high temperature NO2(g) → NO(g) + 1/2 O2(g) is a second...
The decomposition of NO2 at high temperature NO2(g) → NO(g) + 1/2 O2(g) is a second order process with a rate constant of 3.40 L/mol•min. If an experiment is performed where the initial concentration of NO2 is 0.400 M, what is the concentration of NO2after 2.96 min? [NO2] = M
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order...
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order in NH NO2 with a rate constant of 4.70x10-55-1 If the initial concentration of NH_NO2 is 0.902 M, the concentration of NH2NO2 will be M after 45290s have passed In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N205(8) +2 NO2(g) + O2(g) the concentration of N2O5 was followed as a function of time It was found that a...
Write a rate law for the reaction. Write a rate law for the reaction. Rate=k Rate=k[A]...
Write a rate law for the
reaction. Write a rate law for the reaction. Rate=k Rate=k[A]
Rate=k[A]2 Rate=k[A]3
Exercise 14.40 - Enhanced - with Feedback 10 of 32 > A Review | Constants Periodic Table The following reaction is first order in N, 0, N20(g) NO: (C) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. What would the rate of the reaction be at the same concentration as in Part A if the reaction...
Question #: 13 The metal-catalyzed decomposition of N2O was studied to determine the overall order of the reaction. 2 N2O(g) +2 N2(g) + O2(g) As the reaction of N20 was monitored, half of the N20 reacted at 15 seconds, and all the remaining N20 reacted in the next 15 seconds. What is the order of the reaction? A. zeroth-order B. first-order C. second-order D. third-order
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order in NH NO2 with a rate constant of 4.70x10-55-1 If the initial concentration of NH_NO2 is 0.902 M, the concentration of NH2NO2 will be M after 45290s have passed In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N205(8) +2 NO2(g) + O2(g) the concentration of N2O5 was followed as a function of time It was found that a...
Write a rate law for the
reaction. Write a rate law for the reaction. Rate=k Rate=k[A]
Rate=k[A]2 Rate=k[A]3
Exercise 14.40 - Enhanced - with Feedback 10 of 32 > A Review | Constants Periodic Table The following reaction is first order in N, 0, N20(g) NO: (C) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. What would the rate of the reaction be at the same concentration as in Part A if the reaction...
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