Consider the leaching of CuO at 28°C. Using the pH of the solution taken at different periods of time, solve for the reaction rate order and rate constant of the following reaction: CuO+2H+ Time (min) Cu2+ + H₂O pH 0 0 3 0.05 6 0.12 9 0.23 12 0.34 15 0.45 18 0.56 What is the activation energy if the Arrhenius constant is equal to 80,000?

tab lock atrol D esc Question 14 Based on the initial-rate data below, which is the magnitude (units omitted) for the specific-rate constant for this reaction? Rate (M/s) 1.3 x 10-7 5.2 x 10-7 1.0 x 10-6 [HgCl2] (M) [C2042-] (M) 0.10 0.10 0.10 0.20 0.20 0.20 O 5.2 x 10-6 O 1.3 x 104 O 1.3 x 10-5 O 2.0 x 10-7 Question 15 ! An chemical reaction has specific-rate constant 1.10 x 104 s¹ at 470 C. How many hours are required for a 0.335 M solution to decrea to 0.051 M? 1 O A B Ā N @ 2 W S X 2 option command w # E D DS 4 C R TI % 5 V 2 T G > A 6 MacBook Pro CO B Y 4) & 7 H U N 00 8 J - M ( 9 K O ) O < H 5 L P command

A particular 1st-order reaction with a single reactant, whose initial concentration is 0.87 M, has a rate constant of 8.54 s–1. Determine t½ for this reaction. Group of answer choices 0.31 0.089 1.8 1.3 0.081

Time (h) IN,0,1 (mel/1) Time (h) DN0) (mel/L) 0.00 0.849 3.00 0.352 0,50 0.733 4.00 0.262 1.00 0.633 5.00 0.196 2.00 0.472 3. Using data given in the table for the reaction N,O, 2 NO, + 0, calculate the average rate over the interval 0 to 5.0h. Compare your result with the average rates over the intervals 1.0 to 4.0 h and 2.0 to 3.0 h, all of which have the same midpoint (2.5 h from the start).

Consider the following balanced chemical equation: H₂O2 (aq) + 31 (aq) + 2 H* (aq) → 13¯ (aq) + 2 H₂O (1) In the first 49.9 seconds of the reaction, the concentration of 13 increased from 0.692 M to 0.93 M. What is the average reaction rate over this time interval (in mol L-¹ s-¹)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:

Consider the reaction  I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate  (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047

Consider the table of data collected for the reaction A – Products. -> Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.750 0.50 0.665 1.00 0.575 1.50 0.490 2.00 0.410 2.50 0.320 3.00 0.235 3.50 0.150 4.00 0.060

Match the quantities that yield straight lines for the given types of reactions molarity vs. time zero order rate equations inverse molarity vs. time secondorder rate equations In molarity vs. time firstorder rate equations inverse molarity vs. inverse time not a straight line for any type & へ へ

A mechanism was developed to explain the kinetics of the reaction;OCl– + H2O <-------> HOCl + OH– (fast equilibrium)I– + HOCl --------> HOI + Cl– (slow)OH– + HOI ------------> H2O + OI– (fast)Does the rate expression of this mechanism support or refute the data?Is there a catalyst for this reaction? Identify itIs/are there a reaction intermediate(s)? Identify it

The following kinetic data were obtained for the reaction A (g)   +   2 B (g)   →    products   Trial [A] (M) [B] (M) Initial Rate (M s-1) 1 0.60 0.30 0.0126 2 0.20 0.30 0.0014 3 0.60 0.10 0.0042   Determine the order with respect to A. Enter the answer as a single digit, not the word.