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- H20 -OH H30* (1) XS LIAIH4 (2) H2O HO, он (1) XS CH;MgBr (2) H20met (b) Find the forward (k, Jand reverse (k-) rate constants for the recombination kuk-s reaction; OH +H* H20 at 25 °C, 40)-0.51 x 1016 M1 Given: K, = LHOM.H)For an enzyme -catalyzed reaction, KM=10.0 mmol dm-3, vmax=0.250 mmol dm²³ s-'; [E]o= 2.3 x 10-6 mmol dm-3. Calculate the catalytic efficiency (=kb/KM) of the enzyme. 0.920 dm³ mol-l s-1 3.1 x 107 dm³ mol-1 s-1 1.1 x107 dm³ mol-l s-1 0.250 dm³ mol-l s-1
- The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as k = Ae-E/RT where R is the gas constant (8.314 J/mol K), A is a constant called the frequency factor, and Da is the activation energy for the reaction. However, a more practical form of this equation IS In = (1-12) Ea R which is mathmatically equivalent to In Ea F (1/2 R T₂ k2 T1 where ki and k2 are the rate constants for a single reaction at two different absolute temperatures (T₁ and T₂). ▼ Part A The activation energy of a certain reaction is 42.1 kJ/mol. At 20 °C, the rate constant is 0.0150s¹. At what temperature in degrees Celsius would this reaction go twice as fast? Express your answer with the appropriate units. T₂ = Submit Part B Value k₂ = Request Answer Submit Given that the initial rate constant is 0.0150s¹ at an initial temperature of 20 °C, what would the rate constant be at a temperature of 200. °C for the same reaction described in Part…(b) The reaction between H2O2 and lodide; H,0, + 21 + 2H*→ 2H,0 + 12 Proceeds by two parallel mechanism and led to a rate laws, k, [H,0][I] and = k, [H,0][][#*] %3D dt dt The change in observed rate constants with ionic strength for both the mechanisms is given in the following table. k (M's) 0.69 k2 (M's') Sr. no. Ionic strength (1) 19.0 0.00 0.0207 0.66 15.0 3 0.0525 0.67 12.0 4 0.0925 0.68 11.3 0.69 0.1575 0.2025 9.7 0.71 9.2 With the help of this data and corresponding plots, comment on which mechanism between these two would follow Primary salt effect more prominently. rhich tyne of complex mechanism T-jumpIn a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °CCH3NC(g)CH3CN(g)the concentration of CH3NC was followed as a function of time.It was found that a graph of ln[CH3NC] versus time in seconds gave a straight line with a slope of -4.38×10-3 s-1 and a y-intercept of -2.83 . Based on this plot, the reaction is ______ order in CH3NC and the half life for the reaction is _______ seconds.
- The reaction of ethyl acetate with sodium hydroxide, CH3 COOC,H; (aq) + NaOH(aq) = CH3COONA(aq) + C2H; OH(aq) is first order in CH3 COOC,H; and first order in NaOH. If the concentration of CH3 COOC2H; was increased by half and the concentration of NaOH was increased by four, by what factor would the reaction rate increase? Express your answer numerically.Aktiv Chemistry ← → C tab shift + esc caps lock X https://app.101edu.co ! Aktiv Chemistry 40% Phthalonitrile (CHN) is produced by the ammoxidation of o-xylene (C₂H₁) according to the following reaction: 8 C₂H₁(1) + O₂(g) + NH₂(g) → C₂H₂N₂(s) + H₂O(l) 8 10 8 4 How many moles of water would be produced by the complete ammoxidation of 130.0 grams of o-xylene? 2 F2 N W S #3 20 F3 E X 30 $ 4 X + D 8888 F4 R C LO LO % 5 F F5 T Question 12 of 17 V G Y 7 F7 H B U 00 DII F8 J F9 K 4 N M +/- 1 7 70 I F10Given that the reaction of C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (1) AH = - 1411 kJ What would AH be for 2 CO2 (g) + 2 H2O (1) → C,H4 (g) + 3 O2 (g) () 1411 J -1411 J O-1411 kJ 1411 kJ
- The gas-phase decomposition of di-tert-butyl peroxide. (CH₂) COOC(CH3)3, is first order in the temperature range 110°C to 280°C with a first- order rate coefficient k=3.2 x 10¹ exp[-(164 kJ mol/RT³ Part A What is the value of AH for this reaction in the temperature range between 110 Cand 280 C Express your answer with the appropriate units. ΔΗ" - 164 НА kJ mol Submit Previous Answers Request Answer Xncorrect; Try Again; 4 attempts remaining ?[References) Use the References to access important values if needed for this question. In a study of the gas phase decomposition of dimethyl ether at 500 °C CH;OCH;(g)- →CH4(g) + H2(g) + CO(g) the concentration of CH,OCH, was followed as a function of time. It was found that a graph of In[CH,OCH] versus time in seconds gave a straight line with a slope of -6.28x10s and a y-intercept of -3.50 Based on this plot, the reaction i Đ order in CH,OCH, and the rate constant for the reaction is zero first second Submit Answer Try Another Version 2 item attempts remaining (Previous 12 étv ll MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ #3 $ & * 4 6. 7 8 W E R Y { S G J K く C V ...- ~の * 00 ラ エ B1. A → B +B (rate constant = k1) 2. A +B → C+D (rate constant = k2 3. D → E+F (rate constant = k3) 4. F+A → D + G (rate constant = k Express the net change of [F] and [G]& (select 2 answers) а. d[F] = -k3[D]+k4[A][F] dt b. d[G] = -k4[A][F] dt d[E] = -k3[D] dt d[F] = k3[D]-k4[A][F] С. dt d. d[F] = k3[E][F]-k4[A][F] dt = k4[A][F] dt е. d[E] = k3[D] dt f. d[G] = k4[D][G] %3D dt d[E] = k3[E][F] dt