1. At 803 K the first order decomposition of chloroethane, CH3CH2CC2H4+HCI, has a half-life of 60.8...
Half-life equation for first-order reactions: t1/2=0.693k where t1/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s−1). a) What is the half-life of a first-order reaction with a rate constant of 4.80×10−4 s−1? b) What is the rate constant of a first-order reaction that takes 188 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. c)A certain first-order reaction has a rate constant...
The first order decomposition of HI(g) at a given temperature has a half-life of 5.453 x 101 seconds. What is the rate constant for HI(g)?
How do you calculate the half life for this reaction? The first-order reaction of decomposition of azomethane is given below: At a certain temperature, the rate constant for this reaction equals 3.05 X 10^-3 s^-1. Calculate the half-life of this reaction (in seconds) at the same temperature.
3. The half-life for the first order decomposition of N2O3(g) is 6.00 104 s1 at 20 °C. a) Calculate the rate constant, k, at this temperature. b) What percentage of the N2Os molecules will have reacted after one hour?
The decomposition of phosphine is a first order process with a half life of 37.9 s. What is the rate constant for this reaction? 0.0264 s-1 0.0381 s-1 0.0183 s-1 54.7 s-1 26.3 s-1
Question 6 (18 marks) (a) Given that the rate constant k for the first-order decomposition of compound X is 2.65 x 10-9 s', calculate the percentage of compound X that has decomposed in the first 2250 seconds after the reaction begins. (4 marks) (b) Consider the first order reaction: W2 → 2 Y. If [W2]=0.8 M initially and 0.17 M after 160 seconds, what will [W2] be after 350 seconds? (4 marks) (c) Data for the reaction 3A + 5B...
The decomposition of dimethylether at 504o C is first order with a half-life of 1570 seconds. What fraction of initial amount of dimethylether remains after 4710 seconds
The first-order decomposition of hydrogen peroxide has a half-life of 10.7 h at 20°C. a. What is the rate constant (expressed in hr−1) for this reaction? _____________ Write answer to three significant figures and NO UNITS in answer. b. If you started with a solution that was 7.5 × 10−3 M H2O2, what would be the concentration of H2O2 after 3.3 h? __________
The decomposition reaction of A to B is a first-order reaction with a half-life of 6.19×102 seconds: A → 2B If the initial concentration of A is 0.147 M, how many minutes will it take for the concentration of A to be 18.5% of the initial concentration?
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...