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Chemistry
- The initial rate of the reaction between AA and BB was measured. From the data given,a. determine the order of each reactant,b. determine the order of the reaction,c. write the rate law andd. calculate the rate constant, k. Experiment A B initial rate #1 0.20M 0.10M 3.50x10-3M/s #2 0.40M 0.10M 7.00x10-3M/s #3 0.40M 0.40M 7.00x10-3M/s if a reaction is second order in B and the concentration of B increased from 0.0850M to 0.2975M, what should happen to the rate?arrow_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_forwardQuestion:Consider the following reaction:2A + B → C At a certain temperature and pressure, the rate of this reaction is given by the expression:rate = k[A]²[B] Determine the overall reaction order and the individual orders with respect to A and B.arrow_forward
- Radioactive decay is a process that follows first-order kinetics. The half-life of 36Cl is 3.000e+5 years; how long (in hours) would it take for the amount of 36Cl to decrease to 66.45% of its initial amount? Key Concept: Half-life for first order reaction. t½ = 0.693/k.Strategy: Determine rate constant and then calculate time using integrated first order rate lawarrow_forwardQuestion 4 What is the order of reaction with respect to the individual concentration and over all order of reaction for given rate law expression: Rate (Ms-1) = K[L]5/2[C]1[P]2 /3arrow_forwardWhat are the units of the rate constant, k, in a second- order equation if rate is measured in mol/(L s) and all concentrations are in mol/L? answer options: s–1 L/(mol*s) L2/(mol2*s) mol2/(L2*s)arrow_forward
- Question: A proposed mechanism for the condensation of propanone, (CH3)2CO, is as follows: (picture)Use the quasi-stationary state approximation to find an expression for the rate of product formation. Please show steps and calculations for a better understandingarrow_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_forwardExperiment. Initial [A]. (mol/L) Initial [B] (mol/L). Disappearance of [A] 1. 0.16. 0.15 0.08 2. 0.16. 0.30. 0.30 3. 0.08. 0.30 0.08 what is the magnitude of the rate constant for the reaction?arrow_forward
- The photochemical reaction (i.e., the reaction of hydrogen gas and chlorine gas to produce hydrochloric acid is a zero order reaction. If the concentration of Cl2 gas is 0.029 M at 31.6 seconds, and the rate constant at a certain temperature is 0.00562 M/s, what was the initial concentration of Cl2 gas? (answer in 2 significant figures)arrow_forwardExperiment number [A](M) [B](M) Initial Rate (M/s) 1 0.451 0.885 1.13 2 0.451 1.77 1.13 3 1.35 0.885 10.17 What is the order of the reaction in A?arrow_forwardThe 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_forward
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