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![1:04 PM Sun Feb 5
What is the rate for the second order
reaction A→ Products when [A] = 0.260
M? (k = 0.761 M-¹s¹)
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B
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- The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.The reaction: H2 + I2 = 2HI has an Eactivation = 2000 J/mol. Suppose that it has K=7.5x10-5 M-1s-1 at T=700K, find K at T=800K.
- Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].Given: A + B + C ----> Prods. Find the rate law and k (specific rate constant). [A] [B] [C] initial rate (Ms-1) exp.1 0.20 0.10 0.90 1.8 x 10-2 exp.2 0.10 0.20 0.30 3.0 x 10-3 exp.3 0.20 0.20 0.30 1.2 x 10-2 exp.4 0.20 0.20 0.10 4.0 x 10-3 rate = k[A]x[B]y[C]zTrial [Cl O2] [O H-] Initial rate rxn M/s 1 0.0121 0.25 4.00x10-6 2 0.0242 0.25 2.00x10-6 3 0.0121 0.5 4.00x10-6 4 0.0242 0.75 2.00x10-6 a. Determine the overall order of the reaction if 2 O H- + 2 Cl O2 resulting to products at two hundred ninety eight kelvin b. What is the value of the rate constant? c. What time will it reach in seconds if the chlorine dioxide becomes 1.20 * 10-3 M, starting from 4.00 * 10-3 M
- Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=For the reaction A (g) + B (g) + C(g) → D (g) The following data were obtained at constant temperature: trial [A], M [B], M [C], M Initial Rate, M/s 1 0.0500 0.0500 0.0100 6.25 × 10-3 2 0.1000 0.0500 0.0100 1.25 × 10-2 3 0.1000 0.1000 0.0100 5.00 × 10-2 4 0.0500 0.0500 0.0200 6.25 × 10-3 What is the order with respect to each reactant? Write the rate law. Calculate k (using, for example, trial 1 data).Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=
- Calculate the rate constant, k, for the given data. Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80The equilibrium NH3(aq) + H2O(l) ↔NH4+(aq) + OH−(aq) at 25 °C is subjected to a temperature jump which slightly increases the concentration of NH4+(aq) and OH−(aq). The measured relaxation time is 7.61 ns. The equilibrium constant for the system is 1.78 × 10−5 at 25 °C, and the equilibrium concentration of NH3(aq) is 0.15 mol dm−3. (a) Calculate the rate constant for the forward step. kf = _____________. Just value in 3 sig. fig., normal or exponential format, e.g. type in 1.16E6 meaning 1.16 x 106, must use capital E here. Choose a unit in the next question, must be in one of those.Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
