Our body obtains energy from the combustion of glucose. During this process, glucose is transformed first into fructose. This reaction has an activation energy close to 55 kJ inside our body, where the process is catalyzed by enzimes. Without these catalysts, the activation enerrgy is close to 97 kJ. How many times does the catalyst increase the rate of this reaction in our body at a normal temperature close to 98.6 F (37 °C)? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d 1.8 times 1.2 x 107 times 2.3 x 104 times 780 times X Your answer

Our body obtains energy from the combustion of glucose. During this process, glucose is transformed first into fructose. This reaction has an activation energy close to 55 kJ inside our body, where the process is catalyzed by enzimes. Without these catalysts, the activation enerrgy is close to 97 kJ. How many times does the catalyst increase the rate of this reaction in our body at a normal temperature close to 98.6 F (37 °C)? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d 1.8 times 1.2 x 107 times 2.3 x 104 times 780 times X Your answer

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...

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A certain reaction with an activation energy of 135 kJ/mol was run at 475 K and again at 495 K. What is the ratio of f at the higher temperature to f at the lower temperature? Express your answer numerically using one significant figure.
Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,O,(aq) 2 H₂O(1) + O₂(g) The activation energy for this reaction is 75 kJ.mol-¹. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ.mol-¹. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K
Calculate the rate constant at 168 °C for a reaction that has an activation energy, EA = 21.1 kJ/mol and a rate constant, k = 0.0518 s1 at 28.8 °C. R = 8.314472 J• mor1. K-1. Report your answer to THREE significant figures.
A slightly bruised apple will rot extensively in about 2.5 days at room temperature (23.0°C). If it is kept in the refrigerator at 1.0°C, the same extent of rotting takes about 15 days. What is the activation energy for the rotting reaction?
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A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -3,378.84 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
The energy of activation for a particular reaction is 23.7 kJ/mol. At 16.3 °C the rate constant of the reaction is 3.38 × 10° h. 1 Calculate the temperature (in °C) when the rate constant, k = 1.62 × 10 h. 1 R = 8.314472 J/mol K. Report your answer to THREE significant figures.
The activation energy for the following reaction is 125 kJ/mol, and AE for the reaction is -216 kJ/mol. NO₂(g) + CO(g) → NO(g) + CO₂(g) What is the activation energy for the reverse reaction NO(g) + CO₂(g) → NO₂(g) + CO(g) Please enter your answer as a real number only. (The units should be kJ/mol, but leave that off. Just enter a number like 420.3. But don't enter 420.3. Enter the correct answer.)
Given the same reactant concentrations, the reaction CO(g) + Cl2(g) → COCl2(g) at 249°C is 48.4 times as fast as the same reaction at 169°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
What is the activation energy of a reaction if it has the following rate constants?