•Zero-order reaction is a chemical reaction where the rate does not vary with the increase or decrease in the concentration of the reactants.
Question 11 of 15 Submit What amount of time is required for the concentration of A...
Question 11 of 15 Submi What amount of time is required for the concentration of A to decrease from 0.800 M to 0.200 M in the zero-order reaction A B ? (k = 0.0567 M*s-') 1 2 3 (4 5 6 7 8 9
For the following reaction, the concentration of A and the amount of time required to decrease that concentration to one-half of the initial concentration, (vz, are directly proportional. Therefore, a decrease in concentration of A shows a proportional decrease in the half life, tv2. A products What is the order of this reaction? 2 If the rate constant for this reaction is o.0493 M s-1at 400 C, what is the half-life of this reaction, given an initial concentration of 0.821...
Question 13 of 15 Submit How long will it take for the concentration of A to decrease from 1.25 M to 0.205 for the second order reaction A → Products? (k = 1.52 M-'min-)
Submit The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.245 M. What is the value of k for this reaction? M-1s-1 1 2 3 4 5 6 7 8 9 0 x 10
1. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.160 M? (k = 0.456 M⁻¹ s⁻¹) 2. A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 16.0% of the substance to decompose? 3. How long will it take for the concentration of A to decrease from 0.500 M to 0.100 M in the first-order reaction A → B?...
11 of 15 For a starting concentration of 1.0 M, the concentration after an hour for a first-order reaction where k=1.5x10-35-1 would be O 0.0045 M 04.0x10-6 M O 0.99 M O 0.00 M 12 of 15 What is the concentration of a reactant for a second-order reaction after 5 minutes where k=2.5x10-3Ms-2 if the initial concentration was 0.10 M? O 0.099 M O 0.0025 M O 0.013 M O 0.093 M
A reaction A B has the following time dependence for the concentration of [A] vs time. For t=(0 s, 5 s, 10 s, 15 s, 25 s) the concentration of [A]=(30.00 M, 19.81 M, 13.08 M, 8.64 M, 3.77 M). The initial concentration of [A] is the value at t=0 s. (A)Calculate the values of the rate constant k assuming that the reaction is first order. What is the value of k at 5 s? s-1 What is the value...
Question 11 of 20 Submit What volume (in mL) of 0.300 M HCl would be required to completely react with 5.00 g of Al in the following chemical reaction? 2 Al(s) 6 HCl(aq)2 AICI (aq) 3 H2 (g) mL 1 2 3 X 4 5 6 C 7 8 +- x 100 Tap here or pull up for additional resources
[time] [Z] 4. Suppose the data shown are for the second order reaction: → products. What is the value of the rate constant k? O min 50.000 atm 6.250 3.333 2.273. 5. For a first order reaction (G - products) with k = 0.173 min', suppose a chemist runs the reaction starting with an initial concentration [G]. = 12.0 M. a. How many minutes will it take for [G] to decrease to 4.70 M? b. What [G] will remain after...
. Shelf Life at 24 °C (5 p). Determine the t90 (shelf life) at 24 °C for your unknown. Show all work. First, symbolically state the equation(s) you are using defining all variables. rate constant (k) = -0.0016 M^-1s^-1 [C]o=initial concentration: 0.9228 It is a zero order reaction Abs vs Time 1.000 0.900 0.800 Abs 0.500 y = -0.0016x +0.9189 R = 0.9962 0.400 0.300 0.200 0.100 0.000 50 200 250 100 150 Time (hours)