The activation energy of one of the reactions in a biochemical process is $532611 J {mol}^{- 1}$ . When the temperature falls from $310 K$ to $300 K$ , the change in rate constant observed is $k_{300} = x \times 10^{- 3} k_{310 °}$ . The value of $x$ is
[Given: $\ln 10 = 2.3 R = 8.3 J K^{- 1} {mol}^{- 1}$ ]

Question

The activation energy of one of the reactions in a biochemical process is

532611 J {mol}^{- 1}

. When the temperature falls from

310 K

to

300 K

, the change in rate constant observed is

k_{300} = x \times 10^{- 3} k_{310 °}

. The value of

x

is
[Given:

\ln 10 = 2.3 R = 8.3 J K^{- 1} {mol}^{- 1}

]

Aicharya · Accepted Answer

ln K 2 &#160; K 1 = E a R 1 &#160; T 1 - 1 &#160; T 2 ln K 2 &#160; K 1 = 532611 8 . 3 &#215; 10 310 &#215; 300 where K 2 is at 310 &#160; K &#160; &#38; &#160; K 1 is at 300 &#160; K ln K 2 &#160; K 1 = 6 . 9 = 3 &#215; ln 10 ln K 2 &#160; K 1 = ln 10 3 K 2 = K 1 &#215; 10 3 K 1 = K 2 &#215; 10 3 So

The activation energy of one of the reactions in a biochemical process is 532611   J   mol - 1 .…

Solution

The activation energy of one of the reactions in a biochemical process is 532611 &#160; J &#160; mol - 1 .…

Solution

The activation energy of one of the reactions in a biochemical process is 532611 J mol - 1 .…