PH;(2) – P,(2) + H,(2)

3) In the first order "A Product" reaction at 25°C, the initial concentration of compound "A" is 0.8158 M, and its concentration after 15.9 minutes is 0.6311 M. For this first-order reaction, (a) What is the rate constant k, in min? (b) What is the half-life, in min? (c) What will be the molar concentration of "A" after 150 minutes? (d) If the activation energy of this reaction is 34.5 kJ/mol, at what temperature would the half- life of this reaction be 10.0 minutes?

Consider the following reaction: 5Br (ag) + BrO;¯(aq) + 6H*(aq) → 3Br,(aq) + 3H,O() If the rate of disappearance of Br(ag) at a particular moment during the reaction is 3.5×10 mol L-1s-1, what is the rate of disappearance of BrO (aq) at that moment? O 5.8x 10 mol Ls? 07.0x 10 mol Ls! 0 3.5x 10 mol Lis

Which of the following factors would not be expected to affect reaction rate? (A) (B) (C) (D) (E) Adding an appropriate catalyst Grinding up a chunky solid reactant to expose more of its surface area The stability of the reactants (i.e., how stable or how likely a substance is to react) Increase the volume where the reaction would take place Increasing the reaction temperature

(1) The oxidation of ammonia produces nitrogen and water via the following reaction: 4 NH3(g) +3 02(g) → 2 N2(g) +6 H₂O(1) If rate of formation of H2O(7) is 3.0 mol/(L. s) is, (a) What is the rate of formation of Nitrogen gas? (b) What is the rate of disappearance of Ammonia gas?

H2 reacts with ClF. Someone thinks this is the mechanism:                               H2(g)  +  ClF(g) → HCl(g)  + HF(g)                               HCl(g)  +  ClF(g) →  Cl2(g)   + HF(g) (a)     Write the balanced equation for the overall reaction. (b)  Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e)  If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?

Consider the second-order decomposition of A under the following conditions: The initial concentration of A is 0.161 M and after 117 s the concentration has decreased to 0.111 M. (a) What is the value of the rate constant k? 4.0 M-1*s-1 (b) What is the half-life of the reaction? 4.0

Consider the following balanced chemical equation: H2O2 (aq) + 3 r (aq) + 2 H (aq) >l (aq) + 2 H,O (I) If the concentration of iodide (la) decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s

For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) (a) rate = k (X][Y][Z]² X Y Overall rate = k (X]/[Y]/² [Z] -1 (b) 1/2 X Y Overall (c) rate = k [Y] X Y Overall

c) Calculate its half-life 2. The following data were obtained for the gas-phase decomposition of dinitrogen pentaoxide 2N,O, (g) 4NO, (g) +0; () IN,OJ, (mol / L.) Initial Rate (mol /Ls) 0.0750 8.90 x 104 0.190 2.26 x 10 0.275 3.26 x 10 0.410 4.85 x 10 Defining the rate as -A [N;OJ/A write the rate law and caiculate the value of the rate constant