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Consider the first order reaction, AB2 -> AB + B, which has a first order reaction...
The reaction A→BA→B has been experimentally determined to be second order. The initial rate is 0.0100 M/sM/s at an initial concentration of AA of 0.100 MM. Part A What is the initial rate at [A]=0.400M[A]=0.400M? What is the initial rate at ? 0.00250 M/sM/s 0.160 M/sM/s 0.0100 M/sM/s 0.0400 M/s
The rate constant for the first-order reaction below is 0.0547 s–1. AB If the reaction is begun with an initial concentration of A equal to 0.95 M, what is the concentration of A after 20.51 s? __________M
A first-order reaction has a rate constant at 20 C of 2.75 10–2 sec-1 and Ea is 75.5 kJ/mol. What is the rate constant (in sec-1) at 60C? 8. A first-order reaction has a rate constant at 20°C of 2.75 x 10 sec ? and Es is 75.5 kJ/mol. What is the rate constant (in sec ) at 60°C?
A certain reactant disappears by a first order reaction that has a rate constant K= 3.5x10^-3 s-1. If the initial concentration of the reactant is 0.500 M , how long will it take for the concentration to drop to 0.200 M ? 4. A certain reactant disappears by a first-order reaction that has a rate constant k=3.5 x 10 s. If the initial concentration of the reactant is 0.500 M, how long will it take for the concentration to drop...
The reaction between phenolphthalein and hydroxide ion is first order with respect to the phenolphthalein and zero order with respect to the hydroxide. Calculate the rate constant for this reaction when the instantaneous rate of reaction is 2.5 x 10-5moles per liter per second for a concentration of 0.00250 M for the phenolphthalein. Group of answer choices a. 0.010 M-1 s-1 b. 2.5 x 10-5M/s c. 0.010 s-1 d. 0.010 M-2 s-1 e. cannot be determined from the given information
The reaction AB(aq)→A(g)+B(g) is second order in AB and has a rate constant of 0.0157 M−1⋅s−1 at 25.0 ∘C. A reaction vessel initially contains 250.0 mL of 0.130 M AB which is allowed to react to form the gaseous product. The product is collected over water at 25.0 ∘C. How much time is required to produce 226.0 mL of the products at a barometric pressure of 718.3 mmHg . (The vapor pressure of water at this temperature is 23.8 mmHg.)
At a given temperature, the elementary reaction A↽−−⇀B,A↽−−⇀B, in the forward direction, is first order in AA with a rate constant of 0.0480 s−10.0480 s−1. The reverse reaction is first order in BB and the rate constant is 0.0840 s−10.0840 s−1. What is the value of the equilibrium constant for the reaction A↽−−⇀BA↽−−⇀B at this temperature? What is the value of the equilibrium constant for the reaction B↽−−⇀AB↽−−⇀A at this temperature? ?=K= ?=K=
PLEASE SHOW ALL STEPS FOR COMPREHENSION. The reaction is the first order in [A]. Consider the following data: Time [A] M 0.0 1.60 10.0 0.40 20.0 0.10 The rate constant for this experiment is ______ s-1?. A – B
The first order reaction, SO2Cl2 -> SO2 + Cl2, has a rate constant of 0.17 h^-1. If the initial concentration of SO2Cl2 is 1.25 x 10^-3 M, how many seconds does it take for the concentration to drop to 0.31 x 10^-3 M?
Part B AB, has a molar solubility of 3.72 x 104 M. What is the value of the solubility product constant for AB2? Express your answer numerically. View Available Hint(s) O AQ R O 2 ? Kup = Submit