Enter your answer in the provided box. Enter your answer in
scientific notation.
A first-order decomposition reaction has a rate constant of 0.00618
yr−1. What is the half-life of the reaction?
______×10_____yr
For first order reaction....
Half life = 0.693/rate constant
= 0.693/0.00618
= 112.1 year ............. (Ans)
Enter your answer in the provided box. Enter your answer in scientific notation. A first-order decomposition...
Enter your answer in the provided box. The following reaction, 2AB is first order in A and has a rate constant, k, of 7.5 x 10-s-at 110°C. With a starting concentration of [A] = 1.75 M, what will [A] be after 2.5 min? || |м
Enter your answer in the provided box. The reaction 2A → B is first order in A with a rate constant of 2.8 × 10−2 s−1 at 80 ° C. How long (in seconds) will it take for A to decrease from 0.900 M to 0.160 M?
Enter your answer in the provided box. The rate constant of a first-order reaction is 2.35 x 10-45-1 at 350.°C. If the activation energy is 135 kJ/mol, calculate the temperature at which its rate constant is 9.00 x 10-45-1. °c
Be sure to answer all parts. The gas-phase decomposition of peroxyacetyl nitrate (PAN) obeys first-order kinetics: CH3COOONO2 + CH3C000 + NO2 with a rate constant of 4.9 x 10-45-1. Calculate the rate of decomposition (in M/s) if the concentration of PAN is 0.35 ppm by volume. Assume STP conditions. rate= x 100 M/s (Enter your answer in scientific notation.)
Enter your answer in the provided box. What is the half-life in minutes of a compound if 75.0 percent of a given sample decomposes in 30.0 minutes? Assume first-order kinetics.
Enter your answer in the provided box For the simple decomposition reaction ABC) A(g) +B(g) rate= R(AB) and k = 0.20 L/mols. If the initial concentration of AB is 1.50 M, what is [AB] after 12.9
Enter your answer in the provided box. Remember to enter your answer to the correct number of significant figures. For the following reaction, the rate is 0.27 mol/(L·s) when [A]0 = [B]0 = 1.0 mol/L: A(g) + B(g)→ AB(g) If the reaction is first order in B and second order in A, what is the rate when [A]0 = 2.0 mol/L and [B]0 = 3.3 mol/L? PLEASE SHOW WORK
The decomposition of N,is described by the following equation. 2N,O3(2)→ 4NO2(8) + O2(g) If the rate constant is 4.50 x 10-45-1, what is the half-life of this reaction? * 10s (Enter your answer in scientific notation.)
The decomposition of SO2Cl2 is first order and has a rate constant of + 2.90 x 10–4 s–1. What is the concentration of SO2Cl2 after 840 seconds given that the initial concentration of SO2Cl2 is 0.0325M ? (hint: your answer should have three significant figures, not include units, and not be written in scientific notation)
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...