help with this chemistry review ### Initial Rate of Reaction Data AnalysisSome measurements of the initial rate of a certain reaction are given in the table below.| [N\(_2\)] | [H\(_2\)] | Initial Rate of Reaction ||:---------:|:---------:|:------------------------:|| 0.785 M | 0.273 M | 0.859 M/s || 2.30 M | 0.273 M | 2.52 M/s || 0.785 M | 0.347 M | 1.39 M/s |Use this information to write a rate law for this reaction and calculate the value of the rate constant \( k \).1. **Rate Law Expression**: The rate law for a reaction can be expressed in the form: \[ \text{rate} = k [N_2]^x [H_2]^y \]2. **Experimental Data Analysis**: By comparing the initial rates when one concentration is changed while the other is kept constant, you can determine the order of the reaction with respect to each reactant.3. **Calculate the Rate Constant \( k \)**: Rearrange the formula to solve for \( k \): \[ k = \frac{\text{rate}}{[N_2]^x [H_2]^y} \]4. **Significant Figures and Units**: Ensure the calculated value for the rate constant is rounded to 2 significant digits and includes the proper unit.5. **Example Calculation**: Suppose analysis yields the reaction orders \( x \) and \( y \). Substituting the values allows computation of \( k \), which will have the unit \(\text{M}^{-1}\text{s}^{-1}\) or similar, depending on the reaction orders.### Editable Areas:- **Rate Law Expression**: \[ \text{rate} = k [N_2]^x [H_2]^y \] Fill in the determined exponents \( x \) and \( y \).- **Rate Constant \( k \)**: \[ k = \text{value with correct units} \]6. **Graphical/Diagram Descriptions**: The provided image includes an interactive space for calculating and entering

Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.785 M 0.273 M 0.859 M/s 2.30M 0.273 M 2.52 M/s 0.785 M 0.347 M 1.39 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate = & k = x10 X 00 5

Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.785 M 0.273 M 0.859 M/s 2.30M 0.273 M 2.52 M/s 0.785 M 0.347 M 1.39 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate = & k = x10 X 00 5

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Give at least two physical properties that might be used to determine the rate of a reaction.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the following data were obtained: [H2SeO3]0 (mol/L) [H+]0 (mol/L) [I]0(mol/L) Initial Rate (mol/L s) 1.0 104 2.0 102 2.0 102 1.66 107 2.0 104 2.0 102 2.0 10-2 3.33 107 3.0 104 2.0 102 2.0 102 4.99 107 1.0 104 4.0 102 2.0 102 6.66 107 1.0 104 1.0 102 2.0 102 0.42 107 1.0 104 2.0 102 4.0 102 13.2 107 1.0 104 1.0 102 4.0 102 3.36 107 These relationships hold only if there is a very small amount of I3 present. What is the rate law and the value of the rate constant? (Assumethatrate=[H2SeO3]t)
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
. Account for the increase in reaction rate brought about by a catalyst.
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Why awe elementary reactions involving three or more reactants very uncommon?