H2(g) + 12(g)2HI(g)The reaction between hydrogen and iodine is first order for both reactants.i)Write out the rate equation for the reaction, explaining all of the terms in yourrate equation and give the units.ii)What is the overall order for the reaction?iii)What would be the effect on the rate of reaction of:Doubling the concentration of the hydrogenDoubling the concentration of the iodine

Given -> H2(g) + I2(g) -----> 2HI(g) -> order with respect to H2(g) is first . -> order…

H2(g) + 12(g) 2HI(g) The reaction between hydrogen and iodine is first order for both reactants. i) Write out the rate equation for the reaction, explaining all of the terms in your rate equation and give the units. What is the overall order for the reaction? What would be the effect on the rate of reaction of: Doubling the concentration of the hydrogen Doubling the concentration of the iodine ii) iii)

H2(g) + 12(g) 2HI(g) The reaction between hydrogen and iodine is first order for both reactants. i) Write out the rate equation for the reaction, explaining all of the terms in your rate equation and give the units. What is the overall order for the reaction? What would be the effect on the rate of reaction of: Doubling the concentration of the hydrogen Doubling the concentration of the iodine ii) iii)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 94QRT

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Similar questions

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.
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
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.
Explain what is meant by the average rate of a reaction.
For the reaction of crystal violet with NaOH(aq), the measured rate of reaction is 1.27 106 mol L1 s1 when the concentration of crystal violet cation is 4.13 105 mol/L. (a) Estimate how long it will take for the concentration of crystal violet to drop from 4.30 105 mol/L to 3.96 105 mol/L. (b) Could you use the same method to make an accurate estimate of how long it would take for the concentration of crystal violet to drop from 4.30 105 mol/L to 0.43 105 mol/L? Explain why or why not.
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
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.
The data in the table are for the reaction of NO and O2 at 660 K. NO(g) + O2(g) NO2(g) (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant. (d) Calculate the rate (in mol/L s) at the instant when [NO] = 0.015 mol/L and [O2] = 0.0050 mol/L. (e) At the instant when NO is reacting at the rate 1.0 104 mol/L s, what is the rate at which O2 is reacting and NO2 is forming?
Table 11-2 illustrates how the average rate of a reaction decreases with time. Why does the average rate decrease with time? How does the instantaneous rate of a reaction depend on time? Why are initial rates used by convention?
Based on the diagram in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?

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