Question

A graph plotted between log k vs 1/T for calculating
activation energy is shown by

Answer 1

A graph plotted between log k vs 1/T for calculating  activation energy is shown by

• The minimum amount of energy required to make the atoms or molecules activate in order to make them undergo chemical reaction is called the activation energy.
• For plotting a graph of log k vs 1/T, we need to consider Arrhenius equation,
• k = Ae^{-Ea/RT}
• taking log on both sides, we get,
• log k = log A - Ea/2.303RT
• re-arranging the above terms, we get,
• log k = -Ea/2.303RT + log A
• comparing the above equation with standard equation of straight line, we get,
• y = mx + c
• y = log k
• m = -Ea/2.303R
• x = 1/T
• c = log A
• here, we can notice that, the slope (m) is negative and the y - intercept (c) is positive.
• So, we have, k ∝ 1/T
• Hence the graph is as shown below.

Answer 2

The activation energy is given by $-\frac{ Ea} {RT}$

Explanation:

• According to the Arrhenius equation,

• K= $A\times e^-\frac{Ea} {RT}$

• Taking log_n on both side,

• ln K = $ln A - \frac{Ea} {RT}$

• This equation here is corresponding to the equation of the straight line

• y= mx + c

• Where y is the ln K, x is 1/T and c is the ln A.

• The slope of the equation is$- \frac {Ea} {RT}$

• From this slope, the value of Ea or the activation energy can be calculated.

• So the graph should be ln K vs 1/T.

For more information about activation energy,

brainly.in/question/11622037

What is temperature dependence of activation energy of any reaction?

brainly.in/question/7826425

What is activation energy?