The reaction. pyruvate + NADH+H. lactate + NAD* is catalyzed by the enzyme lacate dehydrogenase. Suppose this reaction in the presence of some lactate dehydrogenase results in the production of 30 µmol per minute of lactate when the concentration of puyruvate is 2 mmol per liter. If the concentration of pyruvate is doubled to 4 mmol per liter, how will the rate of production of lactate change? O it will double to 60 µmol per minute O it will remain the same at 30 umol per minute O it will halve to 15 umol per minute O can't tell

The reaction. pyruvate + NADH+H. lactate + NAD* is catalyzed by the enzyme lacate dehydrogenase. Suppose this reaction in the presence of some lactate dehydrogenase results in the production of 30 µmol per minute of lactate when the concentration of puyruvate is 2 mmol per liter. If the concentration of pyruvate is doubled to 4 mmol per liter, how will the rate of production of lactate change? O it will double to 60 µmol per minute O it will remain the same at 30 umol per minute O it will halve to 15 umol per minute O can't tell

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

Enzymes are important molecules in biochemistry that catalyze reactions. The energy diagram illustrates the difference between a catalyzed reaction and an uncatalyzed reaction. Label the energy diagram. 11 Answer Bank products reactants (substrate) activation energy uncatalyzed reaction reaction progress catalyzed reaction transition state free energy AG for reaction
11. Draw a potential energy diagram for a two-step reaction in which the activation energies are 10 kcal/mol (first step) and 3 kcal/mole (second step), the intermediate is 5 kcal/mol higher in energy than the reactants, and the products are 1 kcal/mol lower in energy than the reactants. Label both axes and positions on the curve that correspond to reactants (R), the intermediate (I), transition states (TS₁, TS₂), and products (P). Indicate the activation barriers with vertical lines and the labels Ea1 and Ea2.
Which of the following changes would most likely increase the rate of a reaction? a. increasing the size of the reactant particles b. decreasing the reaction temperature c. decreasing the concentration of a reactant d. decreasing the activation energy for the reaction
When the amount of substrates (reactants) increases, the reaction rate changes differently in catalyzed and non-catalyzed reactions. Describe this.
True or false? For chemical reactions that occurs in multiple steps, the fastest step in the reaction mechanism requires the most amount of energy to proceed.
A reaction with a catalyst does not produce more than a reaction without a catalyst. It simply yields the product: O at the same rate O more quickly O better O slower
Which of the following is not an example of heterogeneous catalysis? a) 2O3(g) → 3O2(g) has a catalyst of Cl(g) b) CO(g) + 3H2(g) → CH4(g)+H2O(g) has a catalyst of Co(s) c) C2H4(g) + H2(g) → C2H6(g) has a catalyst of Ni(s) d) 2CO(g) + 2NO(g) → 2CO2(g)+N2(g) has a catalyst Rh(s)
Which of the following is true given the information below? 3 H, (g) + N, (g) → 2NH, (g); AH = -22 kcal/mol A) The reaction is endothermic. B) The product is higher in energy than the reactants. C) Heat is released D) The activation energy for the reaction is negative.
For the following reaction: CH3COOCH₂CH3 H₂O CH₂CH₂OH. CH₂COOH a. Write a rate equation in terms of the disappearance of each reactant b. Write a rate equation in terms of the appearance of each product.
Free Energy (kcal/mol) 25 20 15 10 5 0 A \ B A D Reaction progress Use the reaction energy diagram above to answer the following questions. Calculate the activation energy, AG ‡, for the step A to B. kcal/mol Calculate the overall energy change, AGº, for the process B to C. Which step is faster, (a) A to B or (b) C to D? kcal/mol
Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
4. The reaction shown below is part of the glycolytic pathway. The standard free energy change for this reaction is +0.4 kcal/mol. Glucose-6-phosphate (G6P) €→ Fructose-6-phosphate (F6P) C) Steady-state concentrations of these compounds in the cell (at 25°C) are 0.675 mM G6P and 0.0969 mM F6P. In which direction is this reaction allowed to proceed in the cell? (show calculations)