2 2.For the first order reaction 2NOCI -> 2NO + Cl₂, the half life is 2.00 minutes. Theinitial concentration of NOCI is 1.50 M. Answer the following 2 questions. How long would ittake for 60.0 % percent of the initial NOCI to decompose?

Step 1: For a first order reaction:ln(A/A0) = -ktwhere A0 is the initial concentration of reactant,…

Answered: 2. For the first order reaction 2NOCI…

Chemistry

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 94AE: For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at...

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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.
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO. NH4NCO(aq) (NH2)2CO(aq) Using the data in the table: (a) Decide whether the reaction is first-order or second-order. (b) Calculate k for this reaction. (c) Calculate the half-life of ammonium cyanate under these conditions. (d) Calculate the concentration of NH4NCO after 12.0 hours.
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?
The initial concentration of the reactant in a tirst-order reaction A —» products is 0.64 rnol/L and the half-life is 30.0 s. Calculate the concentration of the reactant exactly 60 s after initiation of the reaction. How long would it take for the concentration of the reactant to drop to one-eighth its initial value? How long would it take for the concentration of the reactant to drop to 0.040 mol/L?
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.
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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.
For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
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)
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2. For the first order reaction 2NOCI -> 2NO + Cl₂, the half life is 2.00 minutes. The initial concentration of NOCI is 1.50 M. Answer the following 2 questions. How long would it take for 60.0 % percent of the initial NOCI to decompose?