For an enzyme -catalyzed reaction, Km=10.0 mmol dm³, vmax=0.250 mmol dm3 s-l; [E]o= 2.3 x 10-6 mmol dm3. Calculate the catalytic efficiency (=kb/KM) of the enzyme. 0.920 dm³ mol-l s-1 3.1 x 107 dm³ mol-l s-1 O 1.1 x107 dm³ mol-' s-1 O 0.250 dm³ mol-l s-1

For an enzyme -catalyzed reaction, Km=10.0 mmol dm³, vmax=0.250 mmol dm3 s-l; [E]o= 2.3 x 10-6 mmol dm3. Calculate the catalytic efficiency (=kb/KM) of the enzyme. 0.920 dm³ mol-l s-1 3.1 x 107 dm³ mol-l s-1 O 1.1 x107 dm³ mol-' s-1 O 0.250 dm³ mol-l s-1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The enzyme-catalyzed conversion of a substrate has a Michaelis constant of 0.032 mole dm-3. The rate of the reaction is 0.000205 mole dm-3 sec-1 when the substrate concentration is 0.875 mole dm-3. What is the maximum velocity of this reaction?
Suppose that a certain biologically important reactionis quite slow at physiological temperature (37 °C) in theabsence of a catalyst. Assuming that the collision factorremains the same, by how much must an enzymelower the activation energy of the reaction to achieve a1 x 105-fold increase in the reaction rate?
2HI (g) H2(g) + I2(g)The rate equation for the reaction is rate = k[HI]²At 629 K and at a concentration of 2.00 mol dm-3, the rate of decomposition of hydrogen iodide = 24.0 x 10-5mol dm-3s-2. a)Calculate the rate constant, k, for the reaction at 629K. Give the units .b)Calculate the number of hydrogen iodide molecules that decompose per second in 1 dm³of gaseous hydrogen iodide at 629K (at concentration 2.00 mol dm-3).
The rate of a reaction is increased with the addition of a catalyst as shown in the following diagram: Praducts Reactants Reaction Coordinate Energy
The enzyme-catalyzed reaction has the Michaelis-Menten constant KM=0.02 M. The reaction rate is v = 2 M/s at [S] = 0.05 M. Calculate vmax-
6 I- + BrO3- + 6 H+ ----- 3 I2 + Br- + 3 H2O Rate= k[I-]m[BrO3-]n[H+]p rate= (∆[I2])/(3*∆time) [I-] 0.010M [S2O3-2] 0.0010M H2O [BrO3-] 0.04M HCl 0.10M Starch Indicator (sec.) Volume, ml Volume, ml Volume, ml Volume, ml Volume, ml 1 10 10 20 10 10 1-3 drops 301.90 2 20 10 10 10 10 1-3 drops 213.28 3 10 10 10 20 10 1-3 drops 214.92 4 10 10 10 10 20 1-3 drops 86.45 Temperature of Reaction: _______20 C________ 1. Using the dilution equation (M1V1 = M2V2) calculate the concentration of the I-, BrO3- and the H+ (HCl) in the final mixture just prior to any reaction. 2. Calculate the rate for each experiment as explained in the background information. 3. Using the information above determine the rate law (m, n and p) for the reaction. Show all calculations/reasoning in your notebook. m_____________ n_________________ p…
G.78.
The rate constant of the elementary reaction BH, (aq) + NH (aq) → BH;NH3 (aq) + H2 (g) is k = 1.94 x 10-4L mol¯' s-' at 30.0°C, and the reaction has an activation energy of 161 kJ mol. (a) Compute the rate constant of the reaction at a tem- perature of 40.0°C. (b) After equal concentrations of BH (aq) and NH, (aq) are mixed at 30.0°C, 1.00 × 10ª s is required for half of them to be consumed. How long will it take to consume half of the reactants if an identical experi- ment is performed at 40.0°C?
The compound 1,1-difluoroethane decomposes at elevated temperatures to give fluoroethylene and hydrogen fluoride according to the equation: CH;CHF,(3) CH,CHF(g)+HF(g) i See Periodic Table O See Hint At 460 K, the rate constant for this reaction is k= 5.8 x 10-5-1 and the activation energy is E, = 265 kJ/mol. What is the frequency factor for this reaction?
The Arrhenius equation describes the relationship between the rate constant, k, and the energy of activation, Ea. k = Ae-E, IRT In this equation, A is an empirical constant, R is the universal gas constant, e is the base of natural logarithms, and T is the absolute temperature. According to the Arrhenius equation, at constant temperature, reactions with lower activation energies proceed more rapidly at constant energy of activation. reactions at lower temperatures proceed more rapidly at constant energy of activation, reactions with smaller values of A proceed more rapidly at constant temperature, reactions with lower activation energies proceed less rapidly
An uncatalyzed reaction has an equilibrium constant, Keq, of 50. In the presence of an appropriate enzyme, the forward rate of the reaction increased by 20-fold. What is the equilibrium constant in the presence of the enzyme?
[4] The reaction: 21 (aq) + S2O;²-(aq) → I½(aq) + 2SO,²-(aq) is first order with respect to I and first order with respect to S20g. The rate constant k was determined at different temperatures and a plot of In(k) versus 1/T was constructed resulting in the straight line: y = -5781.8x + 14.1. Assume k has units of M's. (a) Determine the activation energy for this reaction. (b) Calculate the value of k at 20 °C.