Nitric oxide decomposition occurs through two parallel reactions NO (g) → ¹½ N2 (g) + ¹/ 02 (g) NO (g) → ½ N₂0 (g) + ¹4 02 (g) k₁= 25.7 S-1 k₂= 18.2 S-1 a. Which reaction is the slow reaction? b. What is the reaction order for these reactions? c. After 0.1 seconds, what is the concentration of N₂ (g) if the initial concentration of NO (g) is 2.0 M?.. d. After 0.025 seconds, what is the concentration of N20 (g) if the initial concentration of NO (g) is 4.0 M?

Nitric oxide decomposition occurs through two parallel reactions NO (g) → ¹½ N2 (g) + ¹/ 02 (g) NO (g) → ½ N₂0 (g) + ¹4 02 (g) k₁= 25.7 S-1 k₂= 18.2 S-1 a. Which reaction is the slow reaction? b. What is the reaction order for these reactions? c. After 0.1 seconds, what is the concentration of N₂ (g) if the initial concentration of NO (g) is 2.0 M?.. d. After 0.025 seconds, what is the concentration of N20 (g) if the initial concentration of NO (g) is 4.0 M?

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Chapter12: Chemical Kinetics

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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.
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
One of the concerns about the use of Freons is that they will migrate to the upper atmosphere, where chlorine atoms can be generated by the following reaction: CCl2F2(g)Freon-12hvCF2Cl(g)+Cl(g) Chlorine atoms can act as a catalyst for the destruction of ozone. The activation energy for the reaction Cl(g) + O3(g) ClO(g) + O2(g) Is 2.1 kJ/mol. Which is the more effective catalyst for the destruction of ozone, Cl or NO? (See Exercise 75.)
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
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.
The dissociation of N2O4 into NO2, N2O4(g)2NO2(g) is believed to occur in one step Obtain the concentration of N2O4 in terms of the concentration of NO2 and the rate constants for the forward and reverse reactions, when the reactions have come to equilibrium.
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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