218 ac D 08 ac dr Solve for the concentration profile at steady state assuming a concentration C =0 as r →∞0 and C=C₁ at r = R (the surface of the sphere).
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- What are the rate laws of mechanisms 1 and 2 for oscillating reactions if the second reactions were the rate-determining steps?Specify the pre-equilibrium and steady-state approximations and explain why they might lead to different conclusions.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)
- he 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,eff = _____________. 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. (b) choose a unit for the forward rate constant. no unit s-1 L/mol/s L2/mol2/sThe 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.The 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,eff = _____________. (b) choose a unit for the forward rate constant. The 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. (c) Calculate the rate constant for the reverse reaction.
- The 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. (c) Calculate the rate constant for the reverse reaction. krev = _____________. Just value in 3 sig. fig., in normal or exponential format, e.g. 1.16E6 meaning 1.16 x 106 must use capital E. Choose a unit in the next question. .The 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,eff = _____________. (b) choose a unit for the forward rate constant. (c) Calculate the rate constant for the reverse reaction. krev = _____________.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.
- The 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 x 10-5 at 25 °C, and the equilibrium concentration of NH3(aq) is 0.15 mol dm-3 (c) Calculate the rate constant for the reverse reaction. Krev = 106 must use capital E. Choose a unit in the next question. Just value in 3 sig. fig., in normal or exponential format, e.g. 1.16E6 meaning 1.16 xManfred Eigen, a German physical chemist working dur- ing the 1970s and 1980s, earned a Nobel Prize for devel- oping the "temperature-jump" method for studying kinetics of very rapid reactions in solution, such as proton transfer. Eigen and his co-workers found that the specific rate of proton transfer from a water molecule to an ammonia molecule in a dilute aqueous solution is k = 2 x 10° s-'. The equilibrium constant Kµ, for the reaction of ammonia with water is 1.8 x 10-8, What, if anything, can be deduced from this information about the rate of transfer of a proton from NH; to a hydroxide ion? Write equations for any reactions you mention, making it clear to which reaction(s) any quoted constant(s) apply.The equilibrium NH3(aq) + H2O(1)→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 x 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,eff= 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.
