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miv72 [106K]
3 years ago
13

7.no . with steps please anyone no spam

Chemistry
1 answer:
gulaghasi [49]3 years ago
6 0
  • Given mass=1.3g
  • Atomic mass=65u

Molar mass=65g/mol

Now

\boxed{\sf No\:of\:moles=\dfrac{Given\:Mass}{Molar\:Mass}}

\\ \rm\longmapsto No\:of\;Moles=\dfrac{1.3}{65}=0.02mol

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the calculated value is Ea is 18.2 KJ and A is 12.27.

According to the exponential part in the Arrhenius equation, a reaction's rate constant rises exponentially as the activation energy falls. The rate also grows exponentially because the rate of a reaction is precisely proportional to its rate constant.

At 500K, K=0.02s−1

At 700K, k=0.07s −1

The Arrhenius equation can be used to calculate Ea and A.

RT=k=Ae Ea

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At 500 K,

ln0.02=lnA+500R−Ea

500R Ea (1) At 700K lnA=ln (0.02) + 500R

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Adding (1) to (2)

700REa100R1[5Ea-7Ea] = 0.02) +500REa=0.07) +700REa.

=ln [0.02/0 .07]

Ea= 2/35×100×8.314×1.2528

Ea =18227.6J

Ea =18.2KJ

Changing the value of E an in (1),

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A=antilog (1.0889)

A=12.27

Consequently, Ea is 18.2 KJ and A is 12.27.

Learn more about Arrhenius equation here-

brainly.com/question/12907018

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