Practice ProblemATTEMPT
The reaction
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Chemistry
- The reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0180 M-1·min-1 at a certain temperature.If the initial concentration of A is 0.580 M. What will be the concentration of A after 58.0 min?Answer MHow long would it take for 66.0% of the starting material (A) to undergo reaction?Answer minarrow_forwardThe reaction A → products is first order. If the initial concentration of A is (6.0400x10^-1) M and, after (9.30x10^1) seconds have elapsed, the concentration of A has fallen to (2.710x10^-1) M, what is the rate constant of the reaction? Answer: ______x10 ____ units____arrow_forwardIn the presence of excess thiocyanate ion, SCN-, the following reaction is first order in chromium(III) ion, Cr3+ Cr3+(aq) + SCN(aq) → Cr(SCN)2+(aq) The rate constant for the reaction is (3.10x10^0)x10-6/s. What is the half-life, in seconds, for the reaction? Express yoyr answer to three significant figures.arrow_forward
- PRACTICE ANOTHER Identify the reaction intermediate or intermediates in the following multi-step mechanism. (Separate substances in a list with a comma.) Overall: 4 NO + 3 O2 + 2 H2O → 4 HNO3Step 1: 2 NO + O2 → 2 NO2Step 2: 4 NO2 + O2 + 2 H2O → 4 HNO3 ??????arrow_forwardThe reaction, A → products, is known to be zeroth order with respect to the concentration of A and zeroth order overall. The rate constant for the reaction is 0.1400 M·hr-1 at a certain temperature.If the initial concentration of A is 0.750 M. What will be the concentration of A after 3.8 hr?Answer MHow long would it take for 95.0% of the starting material (A) to undergo reaction?Answer hrarrow_forwardA reaction that is first order in X has a rate constant of 1.6x10^-2 s^-1. If the initial concentration of X is 1.0 M, what is the concentration of X after 205 s? Please show set up of work so I can understand how to do question. Thank you .arrow_forward
- 2. The initial rate data for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is shown in the following table. Experiment [N2O5](M) Rate (M/s) 1 1.28 × 102 22.5 2 2.56 x 102 45.0 a. Determine the order of reaction of the given reactant. b. Determine the value of the rate constant for this reaction.arrow_forwardIssue 5The data in the table below was compiled for the following reaction. A + B → C + D At temperature T, the following initial velocity data was obtained. Experience [A] (mol/L) [B] (mol/L) Initial speed (mol/L s) 1 0,020 0,020 5,0 x 10-3 2 0,040 0,020 1,0 x 10-2 3 0,040 0,060 4,5 x 10-2 Determine the rate law equation and the rate constant at temperature T with the appropriate units.arrow_forwardA first-order reaction has a half-life of 18.0 seconds. How long (in seconds) will it take for the concentration of the reactant in the reaction to fall to one-eighth of its initial value? (answer in 3 significant figures)arrow_forward
- The gas-phase decomposition of NO2, 2NO2(g) → 2NO(g) + O2(g), is studied at 383 °C, giving the following data: Is the reaction first order or second order with respect to the concentration of NO2? (clue:draw graphs) b) What is the rate constant? c) what is the half-life?arrow_forwardA second order reaction (A --> products) has a rate constant of 6.2 x 10-4 M-1s -1 . If the initial concentration of A is 0.400 M , what will the concentration be after 18 minutes ( 1080 sec)? (Answer has 2 sig figs. don't include units)arrow_forwardCarbon-14 dating is a first order process used to determine the age of artifacts that were made from organic (carbon-containing) materials. Given a rate constant of 1.21 x 10-4 years-1, what is the half life of carbon-14 (i.e., how many years will it take for the initial concentration of carbon-14 in a sample to be reduced to one-half the initial amount)? (answer in 4 significant figures)arrow_forward
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