Consider the following reaction: A + B --> products. The rate law was found to be rate = k[A][B]^2. If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the equation? How will this affect the time required for the reaction to reach completion?

2NH₂(g) → N₂(g) + 3H₂(g) She fills a reaction vessel with NH3 and measures its concentration as the reaction proceeds: time (minutes) 0 1.0 2.0 3.0 4.0 [NH₂] 0.600M 0.324M 0.175M 0.0942 M 0.0508 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X 4

Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,O,(aq) 2 H₂O(1) + O₂(g) The activation energy for this reaction is 75 kJ.mol-¹. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ.mol-¹. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: O [A] = 6.0 and [B] = 0.6 O [A] = 3.0 and [B] = 0.6 O [A] = 4.5 and [B] = 0.6 [A] = 1.5 and [B] = 1.2 O [A] = 3.0 and [B] = 1.8 [A] = 1.5 and [B] = 1.8 O [A] = 3.0 and [B] = 1.2 O [A] = 7.5 and [B] = 0.6 Rate = K[A][B][C] Rate = K[A][C] Experiment [A] (M) [B] (M) Rate (M/s) (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]* [B]Y? Choose all correct possibilities. k[A]² [C] O Rate = K[A][C]² Rate = k[A]²[C]² Rate = k[A]³ [C] O Rate = K[A][C]³ 1 2 Rate = 1.5 3.0 (b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 9, doubling the concentration of B has no effect on the rate, and doubling the concentration of C…

The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3

For the reaction AB(g) —>A(g) + B(g) the rate law is determined to be rate =k[AB]^2 and k=0.255 L/mol-min. If the initial concentration of AB is 1.00M, how long will it take for the concentration of AB to fall to 0.40M?

The data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =

Some measurements of the initial rate of a certain reaction are given in the table below. [H,] [1] initial rate of reaction 0.178M 2.10M 7.00 x 10°M/s 0.0727M 2.10M 2.86 x 10°M/s 0.178M |3.23M 1.08 × 10*M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| x10 k =

The concentration of A was monitored for the reaction A → P and the following data were obtained. What is the rate law, rate = k [A]x, for this reaction?   [A] (M) Time (s) 0.0200 0 0.0169 100 0.0142 200 0.0120 300 0.0101 400 0.0086 500 0.0072 600 0.0061 700     Question 15 options:   rate = 1.7 x 10–3 [A]   rate = 2.3 x 10–3 [A]2   rate = 0 54 [A]   rate = 1.3 x 10–3 [A]     rate = 0 54 [A]2

Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction [N:] H, initial rate of reaction 1.65 M 1.22 M 87.0 M/s 1.65 M0.320 M 5.99 M/s 2.94 M 1.22 M 155. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. x10 rate = %3D k = 0