#14 Rate Constant and Temperature
1. The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T (in K) is linear and has a slope of -1.01 x 104 K. Calculate the activation energy for this reaction.
2. The rate constant of a reaction at 32.0oC is 0.0550 s-1. If the frequency factor is
1.20 x 1013 s-1, what is the activation energy?
3. A reaction has a rate constant of 0.000122 s-1 at 27.0oC and 0.228 s-1at 77.0oC.
a. Determine the activation energy for this reaction.
b. What is the value of the rate constant at 17.0oC?
4. A slightly bruised apple will rot extensively in about 4.00 days at room temperature, 25.0OC. If the same apple is kept in the refrigerator at 5.0OC, the same extent of rotting takes about 16.0 days. What is the activation energy for the rotting reaction?
Ans:) Activation energy is a a enrgy that must be given to a system to initiate or start that reaction.In this question basically the arhenius equation is used most. If their is any doubt please ask in commengt section and life if it helps you.
Thank you !
#14 Rate Constant and Temperature 1. The rate constant (k) for a reaction was measured as...
4. A slightly bruised apple will rot extensively in about 4.00 days at room temperature 25.0°C. If the same apple is kept in the refrigerator at 5.0°C, the same extent of rotting takes about 16.0 days. What is the activation energy for the rotting reaction?
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
A slightly bruised apple will rot extensively in about 2.0 days at room temperature (26.C). If it is kept in the refrigerator at 1.5 C, the same extent of rotting takes about 17 days. What is the activation energy from the rotting reaction? ...................... J/mol fyi( 5.9 J/mol was marked as wrong)
the rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T(in K) is linear and has a slope of -9.90•10^3 K. calculate the activation energy for the reaction.
The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T(in K) is linear and has a slope of −1.12×104 K . Calculate the activation energy for the reaction. Express your answer using three significant figures with the appropriate units.
The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T(in K) is linear and has a slope of -7893 K . Part A Calculate the activation energy for the reaction. Express your answer to four significant figures and include the appropriate units.
The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T(in K) is linear and has a slope of −1.30×104 K . You may want to reference (Page) Section 14.5 while completing this problem. Calculate the activation energy for the reaction. Express your answer using three significant figures with the appropriate units.
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...
The following data show the rate constant of a reaction measured at several different temperatures. Temperature (K) Rate Constant (1/s) 310 4.54×10−2 320 0.136 330 0.381 340 1.01 350 2.51 Part A Use an Arrhenius plot to determine the activation barrier for the reaction. Express your answer using three significant figures. Part B Use an Arrhenius plot to determine the frequency factor for the reaction. Express your answer using two significant figures.
The rate constant k for a certain reaction is measured at two different temperatures: temperature 148.0°C 78.0°C k 9.7x10? 9.4 x 10° Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. 9.- Omol