Question

The activation energy of a reaction can be determined from
the slope of which of the following graphs ? [2015]
(a) ln K/T vs.T
(b) ln K vs. l/T
(c) T/lnK T vs. l
(d) ln K vs . T

Answer 1

The activation energy of a reaction can be determined from the slope of ln K vs. 1/T graph

• We need to find the activation energy of a reaction using slope of the graph.
• we have,
• the Arrhenius equation given by
• $ln K= ln A -\dfrac{E_a}{RT}$
• in this above equation, the slope is given by,
• $=\dfrac{-E_a}{R}$
• Hence the activation energy,
• $E_a=-slope * R$

Answer 2

ln K vs. l/T is the answer.

Explanation:

• According to the Arrhenius equation,

• K= $A \times e^{-Ea/RT}$

• 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  $- \frac{Ea} {R}$

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

• So the graph should be ln K vs 1/T.

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