In the first order reaction A → products, [A] = 0.398 mol/L initially and 0.185 mol/L after 17.0 min. What is [A] after 250 min, in mol/L?
The Integrated rate equation for first order raction is used to calculate the final concentration after 250 min of reaction...
In the first order reaction A → products, [A] = 0.398 mol/L initially and 0.185 mol/L...
In the first order reaction A---> products, [A] = 0.400 M initially and 0.250 M after 15.0 min. What is the value of the rate constant, k?
The reaction A --> Products is second order with a rate constant of 0.2500 L mol-1 s-1. If we start with a 1.000 M concentration of A, what is the rate of the reaction (in mol L-1 s-1) after 20 s? Your answer should be rounded up to four decimal places.
The reaction A--> B is first order in A. Initially [A]= 0.800M and after 54 min., [A]=0.100M. At what time (in min.) is [A]=(2.0e-2)M?
A gas decomposes to form O2 and two other products, in a first-order reaction, with rate constant k = 6.95 x 10 –4/s at 40oC. If the initial gas concentration = 4.80 x 10 –2 mol/L, what is the concentration (M) after 250 seconds have passed?
What statement is true? For the first-order reaction, A → products, 12.5% of initial amount of A is left after two half-lives. For the first-order reaction, A → products, if half of the initial concentration of A reacts in 20 min, then the remaining half will completely react in the next 20 min. For the first-order reaction, A → products, 25% of initial amount of A is left after two half-lives. For the first-order reaction, A → products, 75% of...
[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...
Referen The initial concentration of the reactant in a first-order reaction A → products is 0.528 mol/L and the half-life is 27.0 s. (a) Calculate the concentration of the reactant (in mol/L) 54.0 s after initiation of the reaction. moll (b) How long (in s) would it take for the concentration of the reactant to drop to one eighth its initial value? (e) How long (ins) would it take for the concentration of the reactant to drop to 0.0330 mol/L?...
The concentration of N2O5 is initially 0.500 mol/L. After 100 s it has dropped to 0.250 mol/L and after 200 s it has dropped to 0.125 mol/L. What is the concentration after 150 s? Use the first order concentration-time equation to determine [N2O5] remaining after 150 s.
For the reaction A → products, the data of an experiment in which [A] 0 = 0.6 mol L-1 are: find a) the order of the reaction y) the reaction rate constant c) the reaction half-life. t/min | [AMA]0 100 200 300 400 600 1000 0.829 0.688 0.597 0.511 0.385 0.248 t/min | [AMA]0 100 200 300 400 600 1000 0.829 0.688 0.597 0.511 0.385 0.248
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...