Molecular iodine, I2(g), dissociates into iodine atoms at 625 Kwith a first-order rate constant of 0.271 s-1. (a) What is thehalf-life for this reaction? (b) If you start with 0.050 M I2 atthis temperature, how much will remain after 5.12 s assumingthat the iodine atoms do not recombine to form I2?

The rate constant for this second‑order reaction is 0.630 M−1⋅s−1at 300 ∘C.   A⟶products   How long, in seconds, would it take for the concentration of A to decrease from 0.920 M to 0.290 M?   t= ? s

The gas-phase reaction of NO with F2 to form NOF and Fhas an activation energy of Ea = 6.3 kJ/mol. and a frequencyfactor of A = 6.0 x 108 M-1 s-1. The reaction isbelieved to be bimolecular:NO(g) + F2(g) ----> NOF(g) + F(g)(a) Calculate the rate constant at 100 °C. (b) Draw theLewis structures for the NO and the NOF molecules, giventhat the chemical formula for NOF is misleading becausethe nitrogen atom is actually the central atom inthe molecule. (c) Predict the shape for the NOF molecule.(d) Draw a possible transition state for the formation ofNOF, using dashed lines to indicate the weak bonds thatare beginning to form. (e) Suggest a reason for the low activationenergy for the reaction.

Use the Referénces to access important values if needed for this question. The conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C CH3NC(g)→CH3CN(g) is first order in CH;NC. During one experiment it was found that when the initial concentration of CH;NC was 9.65×102 M, the concentration of CHąNC dropped to 1.43×10-² M after 436 s had passed. Based on this experiment, the rate constant for the reaction is Submit Answer Try Another Version 2 item attempts remaining Previous Nex

Consider the following proposed mechanismHBr + HBr ⇄ H2Br2(fast, equilibrium)HBr + R ⇄ ES(fast, equilibrium)H2Br2 +ES→P+2HBr(slow) (1a) What is the overall reaction? (1b) Identify all catalysts and intermediates in this reaction mechanism. (1c) What is the rate law derived from this mechanism? (1d) If the experimentally determined rate law is rate = k [HBr]3[R]1 what conclusion can be drawn? (1e) If the experimentally determined rate law is rate = k [HBr]2 what conclusion can be drawn? The equilibrium constant (KC) is 10.0 x 10-10 at

For the decomposition of gaseous dinitrogen pentaoxide,2N₂O₅(g) →4NO₂(g) +O₂(g), the rate constant is k=2.8X10⁻³ s⁻¹at 60°C. The initial concentration of N₂O₅ is1.58 mol/L. (a) What is [N₂O₅] after 5.00 min? (b) What frac-tion of the N₂O₅ has decomposed after 5.00 min?

Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s(b) If you start with 0.047 M I2 at this temperature, how much will remain after 5.18 s assuming that the iodine atoms do not recombine to form I2? _______ M

The activation energy (Ea) for the decomposition of a drug was determined to be 43.7 kJ/mol. The rate constant (1) for this decomposition at 60°c was measured as 0.0368 s-1. Which ONE of the following represents (i) the ORDER of reaction and (ii) the pre-exponential factor, 4:

A student obtained the following data for the gas phase decomposition of hydrogen peroxide at 400 °C. H₂O₂(g) H₂O(g) + 2 O₂(g) [H₂0₂], M seconds 0.134 0 6.70x10-² 14.2 ◊ 3.35x10-2 42.7 (1) What is the half-life for the reaction starting at t=0 s? What is the half-life for the reaction starting at t=14.2 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? 1.68x10-2 99.2 (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction? S M-¹S-1

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) the following data were obtained: HI], M seconds 0.274 0.137 6.85×10-2 3.43x10-2 521 782 912 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.274 M is s and when the starting concentration is 0.137 M is (2) The average rate of disappearance of HI from t= 0s to t= 521 s is| Ms!. (3) The average rate of disappearance of HI from t= 521 s to t= 782 s is| Ms! (4) Based on these data, the rate constant for this | | order reaction is Ms!.