Doubling the concentration of a reactant doesn't change the rate of a reaction eight times. With this knowledge, answer the following questions: What is the order of the reaction with respect to that reactant?

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?

The rate of a certain reaction is given by the following rate law: rate = k[NO] [0,] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in 02? What is overall reaction order? At a certain concentration of NO and O2, the initial rate of reaction is 0.270 M / s. What would the initial rate of the M reaction be if the concentration of NO were halved? Round S your answer to 3 significant digits. the reaction is measure — 0.60 М and [O-] The rate to be 62.0 M / s when - 1 - 2 k = ||M [NO] 1.2 M. Calculate the value of the •S rate constant. Round your answer to 2 significant digits.

The rate of a certain reaction is given by the following rate law: rate = k[H,][L] Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in I2? What is overall reaction order? At a certain concentration of H2 and I2, the initial rate of reaction is 93.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 0.290 M/s when [H2] = 1.4 M and [I2] = 1.7 M. Calculate the value of the rate k = constant. Round your answer to 2 significant digits.

Can someone please help with question 3

Consider the following reaction: A (g) + 2B (g) → C (g) + D (g) Is this reaction likely to be an elementary reaction step? Why or why not? Consider what must happen molecularly for the reaction to occur.

If a catalyst was added to this reaction, would it change, not change, increase or decrease the overall order of this reaction

Part C The rate of reaction in terms of the "rate law expression" includes the rate constant (k), the concentration of the reactants, and the orders of the reaction with respect to the different reactants. Consider the following reaction: The initial concentrations of the reactants A and B are 0.200 M and 0.350 M, respectively. The rate of reaction is 0.060 M.s -1, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. -2 -1 Express your answer in M S to three significant figures. ► View Available Hint(s) The rate constant (k) = 1.78 Submit for Part C for Part Cdo for Part Provide Feedback Previous Answers X Incorrect; Try Again; 3 attempts remaining redo for part C reset for Part C keyboard shortcuts for Part C help for Part C M-2.s-1 A+B+C+D

A particular reactant decomposes with a half-life of 151 s when its initial concentration is 0.289 M. The same reactant decomposes with a half-life of 239 s when its initial concentration is 0.183 M. Determine the reaction order. 1 2 0 What is the value and units of the rate constant for this reaction?

Give the characteristic of a first order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant.