1a)
The expression of rate constant (K) according to Arrhenius equation is given by:
............ (1)
Where K is the rate constant, A is the frequency factor or pre-exponential factor, Ea is the activation energy, T is the temperature.
In order to find out the unit of 'A' for the first-order reaction, we have to incorporate the rate equation for the first-order reaction.
We know the expression of the rate constant for the first-order reaction is-
............. (2)
Where t is the time and a is the initial amount of the reactant and x is the amount of product formed after time t.
Now form equations (1) and (2), we will have
Now we know the term has no unit because both 'a' and 'a-x' are representing the same thing.
Hence, the unit of A will be
A = Unit of energy / unit of R * unit of temperature * unit of time
Unit of A = liter mol-1 sec-1
b)
Now we already have:
or
Hence, A is directly related to Ea which is the activation energy. Now we know the greater the collision between the molecules greater will be the activation energy and the value of Ea will be greater as well. Hence as the collision between molecules increases, the value of A should increase and vice-versa.
c)
From the previous equation, we have already got that A is now inversely related to reaction temperature 'T'.
Thus T or reaction temperature has a high effect on the value of A and the value of A decreases as the value of T increases.
d)
Since the term does involve the term T or the reaction temperature, it (T) will have a high impact on the term .
2a)
From the four diagrams, it is clearly visible that the fruitful collisions are only those collisions where the atoms or molecules collide head-on and the atoms or molecules should touch each other. So we can derive the two most important aspects of effective collisions:
1. While getting bombarded, two atoms or molecules must maintain proper orientation.
2. The reactive centers should be as close as possible ( in picture 4, two reactive centers are almost touching one another).
b)
The Arrhenius equation with the probability factor is given by:
Where 'P' is the probability factor
This term 'P', also known as the steric factor, depends on the orientation of the two atoms colliding. The more proper the orientation, higher the value of P will be. Hence, if individual atoms are colliding with proper orientation instead of a molecule, then the value of 'P' should be higher.
I need help please: Reaction Mechanisms and Catalysis 1. The rate constant in an elementary reaction's...
The rate of the elementary reaction C2H2 + O2C2H + HO2 has been studied as a function of temperature between 300 and 2500 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 300 6.25×10-45 740 1.19×10-12 1180 1.91×10-4 1620 1.07 (a) Calculate the activation energy of this reaction. kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol-1 s-1
12) The rate of the elementary reaction CS2 + O2 ---> CS + SO2 has been studied as a function of temperature between 1500 and 2100 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 1500 2.18×104 1620 4.82×104 1740 9.57×104 1860 1.74×105 (a) Calculate the activation energy of this reaction. ___ kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. ___...
Which of the following statements is/are correct? 1) The term e-Ea/RT in the Arrhenius equation is the fraction of reactant molecules having energy less than the activation energy Ea. 2) As a general rule, the probability of correctly oriented collisions between reactant molecules will be low if the molecules are structurally simple, and high if the molecules are complex. 3) The concentration dependence of the rate for an elementary process in a reaction cannot be determined from the stoichiometric coefficients...
the Arrhenius Equation for the rate constant ka zpe is the number of collisions per second, and p is the orientation factor For the reaction A B , z = 1012 collision per second, and p = 0.5. At a temperature T 300.0 K, how many effective collisions occur per second CASO SO,000 17. The rate constant (ka) of a reaction is 3.46 X 102/sec at 298 K. What is the rate constant (kz) at 350.0 K, if the activation...
To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(g)+CO(g)→NO(g)+CO2(g)NO2(g)+CO(g)→NO(g)+CO2(g) does not involve a collision between an NO2NO2 molecule and a COCO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: NO2(g)+NO2(g)→NO3(g)+NO(g)NO2(g)+NO2(g)→NO3(g)+NO(g) NO3(g)+CO(g)→CO2(g)+NO2(g)NO3(g)+CO(g)→CO2(g)+NO2(g) Each individual step is called an elementary step. Together, these...
Need help with the first picture. Data provided in pictures #2 & #3 Determining the Activation Energy and Collision Frequency Factor for Reaction 1 Part 1. Transfer the reaction rate for runs 9.12 from Data Sheet 3. Then calculate the rate constant (R) at each temperature based on the reaction orders determined in parts and Record the results in Tables * = 18,0 ->15.0416"5,0216" Equation 6 ->25 10 2. Calculate the natural logarithm of the rate constant. In ) and...
INFORMATION reaction must also be perimental mea data are plotted in the sult means that the rate Because a reaction is faster at higher temperatures, the rate constant for the reaction m larger. The activation energy of a reaction can therefore be determined from experime surements of the rate constant at several temperatures. When the collected data are ple form In(k) vs T. as shown in Figure 2. a straight line is produced. This result means constant varies exponentially with...
a) Given these data for the reaction , write the rate-law expression. (Use k for the rate constant.) Rate = _______ The specific rate constant = ___________ Expt. Initial [A] (M) Initial [B] (M) Initial Rate of Formation of C () 1 0.15 0.40 4x10^-5 2 0.15 0.80 1.6x10^-4 3 0.30 1.6 1.3x10^-3 b) The rate of the elementary reaction C2H2 + H2->C2H4 has been studied as a function of temperature between 300 and 2500 K. The following data were...
The rate constant for the following elementary reaction is 3.9 times 10^9 M^-2 s^-1 at 25 degree C: 2A(g)+B(g) rightarrow 2C(g) What is the rate constant for the reverse reaction at the same temperature?
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...