Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k O Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for the reverse of the hwo k = 0

estimate the value of the rate constant k

O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. N2 H, initial rate of reaction 2.21 M 2.33 M 35.0 M/s 2.21 M 4.98M 160. M/s 7.27 M 2.33 M 379. 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 O k = | Explanation Check O 2021 McGraw-Hill Educ P Type here to search III

Given the information below, determine the rate law for the reaction and the rate constant (k). Be sure to include the units for the rate constant (k). A + 2B --> C + D [A] M [B] M Initial Rate (M/s) 0.10 0.10 0.0015 0.20 0.10 0.0060 0.20 0.20 0.0120 0.40 0.10 0.0240 rate law: rate constant k:

During a chemical reaction the temperature drops from 26 oC to 14 oC. What can you conclude about the reaction? It has a high activation energy It is a combination reaction It is an endothermic reaction It is an exothermic reaction

The rate law for the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(g) is rate = K[NO]²[H₂] -1 If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 x 10-6 mol L-¹, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 X 9.56 5-1 mol L-¹5-1 L³ mol-³ s-1 3 L² mol-2 s-1 L mol-¹ S-1

Some measurements of the initial rate of a certain reaction are given in the table below. N2|||H2|initial rate of reaction 2.46M 2.06M 0.603M/s 11.3М| 2.06М 12.7M/s 2.46M 5.01М 3.57M/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 ||| k =

Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.619M 0.967 M 2.00 × 105 M/s 0.619M 3.31M 2.97M 0.967 M 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k 2.34 × 10 M/s 9.60 × 105 M/s k = 0 0 x10 ロ・ロ X

Consider the reaction 2HI→ H₂+I2. The rate of disappearance of HI follows the second order rate law. A[HI] = -k[HI]² At The rate constant kis 2.01 x 10-2 M-1s-1. What was the initial concentration of HI (in units of molarity) if the concentration of HI was found to be 0.262 M after t = 45.0 s? Report your answer using three significant figures. Provide your answer below: M rate

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 142.0 °C 6.1 x 1011 226.0 °C 3.7 x 10¹2 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. mol ×