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D Question 7 2 pts How long (in hours) does it take for a first order...
Incorrect Question 9 0/2 pts A first order reaction with a k=0.216 (with units expressed in hours). How long in hours, to have 87.5% of the original concentration remaining. Answer to 2 decimal places. 0.62 Partial Question 6 1.5/3 pts The following reaction was run four times: NO(g) + Cl2le) - NOCIE) What is the order of reaction with respect to: NO- 1/2 C12= 1 Solve for the reaction constant (proportionality constant): k= 1.14 X10 -5 (Answer to 2 decimal...
Question 3 1 pts The rate constant, k, of the first order reaction A B +C is k = 8.62 x 10-35-1. If the initial concentration of A is 2.74 M, how long will it take for the concentration of A to fall below 0.32 M? Give your answer to one decimal place in MINUTES (do not input the units). For example, if your answer is 8.956 minutes, enter 9.0 Question 4 1 pts The rate constant, k, of the...
6. For a first order reaction with k .00021/min, how long would it take for the reactant concentration to drop to one half its original concentration? If you do not have enough information to calculate an answer, what information would you need?
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as 0.693 - 1/2K For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as 1/2 k(Alo Part A A certain first-order reaction (A>products) has a rate constant of 9.60x10 s-1 at45 C. How many minutes does it take for the concentration of the...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t 1/2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t 1/2 = 1 k[A ] 0 Part A A certain first-order reaction ( A→products ) has a rate constant of 9.90×10−3 s −1 at 45 ∘...
2 pts A first order reaction with a k=0.216 (with units expressed in hours). How long, in hours, to have 87.5% of the original concentration remaining. Answer to 2 decimal places. Question 10 1 pts Calculate the Ea (kJ/mol) to 3 significant figures for the reaction: 2HI(g) +H2(g) + 12(e) kq=2.15x108 (1/M x sec) at 6.50x102K(T1) k2-2.39x107(1/Mx sec) at 7.00x102K(T2) R-8.31 J/mol x K) (Hint: you will need to convert this to kJ)
A first order reaction has a half-life of 196 seconds at 25oC. How long (in minutes) does it take for the concentration of the reactant to drop to 3.125% of the original concentration? (it's not 16.34) The rate constant of a chemical reaction increased from 0.197 s-1 to 3.24 s-1 after raising the temperature from 20.0 oC to 60.0 oC. What is the activation energy (in kJ/mol) for this reaction? (Hint: Think about what R value to use and what...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k k and not on the reactant concentration. It is expressed as t1/2=0.693k t 1 / 2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0. A certain first-order reaction (A→products A → p r o d u c t s ) has a rate constant of 9.30×10−3...
A first-order reaction has a half-life of 20.8 s . How long does it take for the concentration of the reactant in the reaction to fall to one-fourth of its initial value?
A certain first-order reaction (A→products) has a rate constant of 1.00×10−2 s-1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25%% of the original concentration? Express your answer with the appropriate units.