In going from room temperature (25.0°C) to 20°C above room temperature, the rate of a reaction...
In going from room temperature (25.0°C) to 20°C above room temperature, the rate of a reaction quadruples (increases by a factor of 4). Calculate the activation energy for the reaction.
The answer is 54.6 kJ/mol but this is not the answer I get
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In going from room temperature (25.0°C) to 20°C above room
temperature, the rate of a reaction...
In going from room temperature (25 C) to 10 C above room temperature, the rate of...
In going from room temperature (25 C) to 10 C above room temperature, the rate of reaction doubles. Calculate the activation energy for the reaction .
If the rate constant of a reaction increases by a factor 2.5 when the temperature is...
If the rate constant of a reaction increases by a factor 2.5 when the temperature is increased from 22 °C to 35 °C, then what is the activation energy (in kJ/mole) of the reaction? A) 5.3x10^4 kJ/mol B) -5.3x10^1 kJ/mol C) 0.45 kJ/mol D) 5.3x10^1 kJ/mol E) -4.5x10^5 kJ/mol
Another reaction has an activation energy of 54.6 kJ/mol. The value of k at 25.0 °C...
Another reaction has an activation energy of 54.6 kJ/mol. The value of k at 25.0 °C is 4.23 × 10−2 s−1. At what temperature will the value of k be 1.15 × 10−2 s−1? Before working the problem, decide if the answer is less than or greater than 25.0 °C.
If the rate constant k of a reaction doubles when the temperature increases from 111 °C...
If the rate constant k of a reaction doubles when the temperature increases from 111 °C to 289 °C, what is the activation energy of the reaction in units of kJ/mol? Do not enter units with your numerical answer. Do not use scientific notation.
Please answer questions 1 and 2 on The rate constant for the reaction answered A +...
Please answer questions 1 and 2
on The rate constant for the reaction answered A + B->C out of 1.0 is 4.1 x104 U(mol s) at 593 K. The activation energy is 101 kj/mol. question Determine the temperature when the rate constant is 1.2 x10-3 L/(mol s)- Answer: 2 One (often inaccurate) rule of thumb in biology is that a 10 °C change increases the rate by a factor of ten. If the lower temperature is 3 °C, what activation...
A slightly bruised apple will rot extensively in about 4.5 days at room temperature (25.0°C). If...
A slightly bruised apple will rot extensively in about 4.5 days at room temperature (25.0°C). If it is kept in the refrigerator at 0.5°C, the same extent of rotting takes about 18 days. What is the activation energy for the rotting reaction? _____ J/mol
The rate constant of a chemical reaction increased from 0.100 s from 25.0 °C to 49.0...
The rate constant of a chemical reaction increased from 0.100 s from 25.0 °C to 49.0 °C to 2.80 s upon raising the temperature Part A Calculate the value of | where Ti is the initial temperature and T, is the final temperature. Express your answer numerically. Calculate the value of In where k, and k, correspond to the rate constants at the initial and the final temperatures as defined in part A. What is the activation energy of the...
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for...
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...
7. In two trials with identical starting concentrations of reactants, the rate increases by a factor...
7. In two trials with identical starting concentrations of reactants, the rate increases by a factor of 3.27 when the temperature is increased from 400 K to 670 K. What is the activation energy for this reaction? Express your answer in kJ / mol. 8. The activation energy for a particular reaction is 4.8 kJ mol-1. The temperature in one trial reaction is 350 K. To what temperature must the reaction be heated to increase the rate constant by a...
Reaction Rates and Temperature 31 Review Constants i Peric The rate constant of a chemical reaction...
Reaction Rates and Temperature 31 Review Constants i Peric The rate constant of a chemical reaction increased from 0.100 - 2005 - pon raising the temperature from 250 C 350 C Learning Goal To use the Athenius equation to calculate the activation energy As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means at a higher percentage of the molecules possess the required activation energy and the reaction goes faster. This relationship is shown...
Please answer questions 1 and 2
on The rate constant for the reaction answered A + B->C out of 1.0 is 4.1 x104 U(mol s) at 593 K. The activation energy is 101 kj/mol. question Determine the temperature when the rate constant is 1.2 x10-3 L/(mol s)- Answer: 2 One (often inaccurate) rule of thumb in biology is that a 10 °C change increases the rate by a factor of ten. If the lower temperature is 3 °C, what activation...
The rate constant of a chemical reaction increased from 0.100 s from 25.0 °C to 49.0 °C to 2.80 s upon raising the temperature Part A Calculate the value of | where Ti is the initial temperature and T, is the final temperature. Express your answer numerically. Calculate the value of In where k, and k, correspond to the rate constants at the initial and the final temperatures as defined in part A. What is the activation energy of the...
Reaction Rates and Temperature 31 Review Constants i Peric The rate constant of a chemical reaction increased from 0.100 - 2005 - pon raising the temperature from 250 C 350 C Learning Goal To use the Athenius equation to calculate the activation energy As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means at a higher percentage of the molecules possess the required activation energy and the reaction goes faster. This relationship is shown...
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