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5. N20 de composes according to 200 2N₂ + O2 The rate of the reaction is...
The decomposition of N,is described by the following equation. 2N,O3(2)→ 4NO2(8) + O2(g) If the rate constant is 4.50 x 10-45-1, what is the half-life of this reaction? * 10s (Enter your answer in scientific notation.)
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
Determine the order for [SO] in the following reaction 2 SO(g) + O2(g) - 2 SO2(g) [SO]i (M) [O] (M) Initial Rate (MS-1) 0.120 0.100 1.50 x 10-3 0.240 0.100 3.00 x 10-3 0.120 0.200 1.20 x 10-2 QUESTION 27 Determine the order for [O2) in the following reaction 2 SO(g) + O2(g) - 2 SO2(g) [SO]i (M) [O2li (M) Initial Rate (Ms-1) 0.120 0.100 1.50 x 10-3 0.240 0.100 3.00 x 10-3 0.120 0.200 1 1.20 x 10-2 QUESTION...
3(12) The first-order reaction, 2N2O(g) + 2N2(g) + O2(g), has a rate constant of 0.76 s at 1000K. (a) Calculate the half-life of this reaction at 1000K. (b) How long will it take for the concentration of N20 to fall to 25% of its initial value at 1000K (c) How long will it take for reaction to be 90% complete? (d) If the half-life of the same reaction is 29 min at 800K, what is the rate constant at 800K?...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
2 5 Consider the reaction: 2N,05 —4N0, +02 This reaction was run, and the following data was obtained. Determine the reaction rate order with respect to the reactant. Time (seconds) 0 600 1200 1800 2400 3000 3600 [N205] 0.0365 0.0274 0.0274 0.0157 0.00860 0.00860 0.00640
3. For the reaction C3H3(g) + 5 O2(g) ----> 3 CO2(g) + 4H20(1) the following rate data were determined at 30°C. Experiment Initial C3H8 Initial O2 id. Rate 0.200M 0.200 M 3.00 x 101 0.400 M 0.200 M 6.00 x 101 0.200 MO 0.400 M 1 .20 x 102 a) Determine the reaction order with respect to C3H8. b) Determine the reaction order with respect to 02. c) Calculate the rate constant at this temperature. d) Write the rate law...
The rate law for the reaction 2NO2 + O3 ? N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 ? N2O4 (fast) N2O4 + O3 ? N2O5 + O2 (slow) B) NO2 + O3 ? NO5 (fast) NO5 + NO5 ? N2O5 + 5/2O2 (slow) C) NO2 + O3 ? NO3 + O2 (slow) NO3 + NO2 ? N2O5 (fast) D) NO2 + NO2 ? N2O2...
When nitrogen gas is combined with oxygen gas to form nitrogen monoxide, according to the reaction N2 + O2 → 2NO, what can be used to measure the rate of the reaction? Group of answer choices: A) N2 consumption B) NO formation C) Both A and B D) O2 production
5. Given the following reaction and the accompanying data: NO2 + 03 ------ NO3 + O2 Exper. Initial [NO2] Initial [03] Initial Rate (mol L* sl) 1 2.3 x 10-5 3.0 x 10-5 1.0 x 10-5 4.6 x 10-5 3.0 x 10-5 2.1 x 10-5 3 4.6 x 10-5 6.0 x 10-5 4.2 x 10-5 Determine the rate law and rate constant for this reaction Rate constant = Answer: Rate =