6B.4 The rate constant for a gas-phase reaction was reported as 6.2 × 10-14 cm³ molecule-1 s-1 at 298 K. What would its value be in cubic decimetres per mole per second?
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6b4: In addition to solving the problem please give brief explanation for concepts and solution if able.
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- 25) Consider the following set of reactions. Assume that A, B, C and D are atoms. (1) A + A → B (2) А-В + С-D А-С-D-B (3) A + B-C → A-B-C Order these reactions in terms of increasing significance of the orientation probability (that is the A in the Arrhenius equation). А. (1) (2) < (3) В. (3) < (2) <(1) C. (1) < (3) <(2) D. (1) = (2) = (3) E. (1) < (2) = (3)2. a) Calculate the hard-sphere (HS) collision theory rate constant ks for the reaction NO(g) + C₁₂(g) Þ NOCl(g) + HS Cl(g) at 300 K in units of dm³ mols. The collision diameters of NO and Cl₂ are 370 and 540 pm, respectively. 16.0 g/mol, and mcı Use masses of m₁ = 14.0 g/mol, mo = 35.0 g/mol. N = b) Now include the line-of-centers (LOC) energy criterion to find koc in units of dm³ mol¹ s¹ using E₁ = 84.9 kJ mol LOC LOC c) Calculate the ratio of kчs and kLoc to the experimental rate constant at 300 K given A = 3.981 10° dm³ mol¹ s and E₁ = 84.9 kJ mol¹. a -120B.2(b) The rate constant for the first-order decomposition of a compound A in the reaction 2 A→P is krr=3.56×10−7 s−1 at 25 °C. What is the half-life of A? What will be the pressure, initially 33.0 kPa after (i) 50 s, (ii) 20 min after initiation of the reaction?
- E17C.1(b) The equilibrium constant for the binding of a drug molecule to a protein was measured as 200. In a separate experiment, the rate constant for the binding process, which is second order overall, was found to be 1.5 x 10 dm mol s. What is the rate constant for the first-order dissociation of the drug molecule from the protein- drug complex?A rate constant is found to fit the expression kr = Ae−(4972 K)/T with A = 4.98 × 1013 dm3 mol−1 s−1 near 25 °C. Calculate Δ‡G for the reaction at 25 °C; assume κ = 1.Hydrogen purification was conducted at 550 °C using a 3-mm-thick palladium sheet having an area of 0.25 m?. (a) Calculate the diffusion coefficient of hydrogen in palladium at this temperature. The preexponent and the activation energy are 12,000 J/mol and 6.5 x 108 m?/s, respectively. R = 8.3145 J/mol-K. (b) When the steady-state condition was attained, hydrogen concentrations at the high- and low-pressures side of the plate were 1.7 and 0.5 kg/m³. Compute the amount of hydrogen that passes through the sheet per hour (in kg/h).
- (a) Consider the following data that have been obtained for the decomposition of N2O5(g) at 67 °C according to the reaction: 2 N2O5(g) 4 NO2(g) + O2(g) [N2O5]/mol dm-3 t/s 0 2.000 120 1.41 240 0.994 360 0.698 480 0.492 600 0.346 (i) Based on the above data, briefly describe two methods which can be used to determine the order of the reaction and the rate constant. (i) Use the methods you described above to determine the order of the reaction and the rate constant. (b) The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³ mol¹¹ at 24°C and 2.01 x 10-2 dm³ mol-¹s¹ at 37°C. Calculate the activation (Ea) energy of the reaction.The rate law for the reaction A + 3B → 2C + D was found to be v = k[A]2[B]2. (a) What are the units of k? (b) Express the rate law in terms of the rates of formation and consumption of A and C, respectively.Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³
- 6.13 Before solving the problem please also give a brief explanation of the concept or associated equation(s) and variables.6c3. Please solve the following problem, give the relevant equation(s) used and explanation.Suppose it is known that ozone adsorbs on a certain surface in accord with a Langmuir isotherm. How could you use the pressure dependence of the fractional coverage to distinguish between adsorption (i) without dissociation, (ii) with dissociation into O + O2, (c) with dissociation into O + O + O?