Give the characteristic of a first order reaction having only one reactant.   A The rate of the reaction is directly proportional to the concentration of the reactant.   B The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.

Determine the rate constant for the reaction 2 A + B - C [A] (M) [B] (M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.56 O 2.8 x 102 M-2s-1 O 14 M-2s-1 O 1.4 x 102 M-2s-1 O 1.4 x 103 M-2s1

11. The graph here shows the concentration of reagent A in a reaction. Which is the best estimate of the initial rate of the reaction? Concentration of A (moles/L) vs Time a) 625 M/s 1.000 b) 16.4 M/s 0,900 c) 0.029 M/s 0.800 0.700 d) 7.40 x 10³ M/s 0.600 0.500 0.400 0.300 0.200 0.100 0.000 60 80 0 20 40 time(s) 100 120

A ---> B  (2nd order)                               Time (sec)      [A]                             0.0           1.60                             10.0         0.40                             What is the rate constant for this reaction? Group of answer choices 5.33Ms .188 Ms 0.40Ms 1.55Ms

Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products   Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3  2 0.115 0.270 2.16 × 10−2  3 0.345 0.135 8.10 × 10−3  What is the order of the reaction with respect to A, with respect to B, and overall?

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

8. Rates for a certain chemical reaction involving the reactant A were measured as a function of the concentration of A, and these data were plotted in the graph below. What is the order of the reaction with respect to A, and what is the rate constant for the reaction? 0.012 0.010 0.008 0.006· 0.004 0.002 0. 0.2 0.4 0.6 0.8 1 [A](M) A) order with respect to A = 0, k = 0.010 s-l B) órder with respect to A = 1, k = 0.010 s C) order with respect to A = 2, k = 0.00 s- D) order with respect to A = 0, k = 10 s E) order with respect to A = 1, k = 100 s- 11:2 a 2/18 Cop Rate (M/s)

Question 9 Which of the following statements is false? The average rate of a reaction decreases during a reaction. It is not possible to determine the rate of a reaction from its balanced equation. The rate of zero order reactions is not dependent on concentration. The half-life of a first order reaction is dependent on the initial concentration of reactant. None of the statements are false.

What is the rate of the reaction when A=0.43M and B=0.31M?

Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1