The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. If k = 6.78 x 10-5 s-1 and the initial concentration of A is 0.57 mol L-1, what is the half life of this reaction in hours?
The following chemical reaction: A → products shows first order kinetics with respect to A; rate...
Question text The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. If k = 6.80 x 10-5 s-1 and the initial concentration of A is 0.63 mol L-1, what is the half life of this reaction in hours?
help please The following chemical reaction: A → products shows second order kinetics with respect to A; rate k[A2 Assume k = 11.88 x 10-5 mol-1 L s-1 If the initial concentration of A is 0.28 mol L-1, what is the concentration of A in mol L-1) after 3.03 hours? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 101" should be entered...
please help me with both. TIA The following chemical reaction: A → products shows zero order kinetics with respect to A; rate = k[A]º. if k = 9.65 x 10-3 moll's and the initial concentration of A is 0.622 mol L-1, what is the half life of this reaction in minutes? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104 should be...
1-The rate constant of a chemical reaction was measured at several temperature values and a plot of ln k (on the y-axis) was plotted against 1/T (on the x-axis, temperature was measured in Kelvin). If the slope of the plot was -9.21 x 103 K and the y-intercept was 13.0, what is the activation energy (EA) of the reaction in kJ mol-1? 2-In an enzyme-catalyzed reaction, the rate of the reaction depends on which of the following at very low...
5. A chemical reaction of the general type A → 2B is first-order, with a rate constant of 1.52 x 10-45-1. a. Calculate the half-life of A. b. Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-
A chemical reaction of the general type: A → 2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a) Calculate the half-life of A. b) Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.
23) A chemical reaction of the general type: A → 2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a. Calculate the half-life of A. b. Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.
Compare and contrast how first-order reaction kinetics and zero-order reaction kinetics differ in terms of the depletion of a reactant A in a chemical reaction. Assume an initial concentration of 420 mg of A. Assume a half-life of 30 minutes if first-order kinetics are obeyed, and a depletion rate of 60 mg/hour if zero-order kinetics are obeyed. Use a clearly drawn graph(s) to determine which rate will result in complete depletion of A over the shortest time. Assume 99% to...
3. A reaction 2A 2B + C is known to follow second-order kinetics, with k = 7.20x10*M's' at 25.0 °C. (20 points) During one experiment, the initial concentration of A is [A]. = 0.120 M (a) Calculate the half-life (1,2), in hours, for this experiment. (b) Calculate the initial reaction rate (in M/s) for this reaction (4 points) (c) How long will it take (in hours) for the concentration of C to reach [C] = 0.0540 M (6 points) (d)...
In a chemical reaction that has first order kinetics, which is true at a constant temperature? A. Half Life and k are both constant B. Neither Half Life nor k is constant C. Half life is constant, but k changes D. Half life changes. but k is constant