3 years ago

Pls somebody help me with this question...

Chemistry

1 answer:

drek231 [11]3 years ago

5 0

It’s B, I think you’re right.

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The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea = 71.0kJ/mo

aleksandrvk [35]

Explanation:

Relation between temperature and activation energy according to Arrhenius equation is as follows.

k = $A exp^{\frac{-E_{a}}{RT}}$

where, k = rate constant

A = pre-exponential factor

$E_{a}$ = activation energy

R = gas constant

T = temperature in kelvin

Also,

$ln (\frac{k_{2}}{k_{1}}) = (\frac{-E_{a}}{R}) \times (\frac{1}{T_{2}} - \frac{1}{T_{2}})$

$T_{1}$ = $244^{o}C$ = (244 + 273) K = 517.15 K

$T_{2}$ = $324^{o}C$ = (597.15 + 273) K = 597.15 K

$k_{1}$ = 6.7 $M^{-1} s^{-1}$ , $k_{2}$ = ?

R = 8.314 J/mol K

$E_{a}$ = 71.0 kJ/mol = 71000 J/mol

Putting the given values into the above formula as follows.

$ln (\frac{k_{2}}{6.7}) = (\frac{-71000}{8.314} \times (\frac{1}{597.15} - \frac{1}{517.15})$

= 2.2123

$\frac{k_{2}}{6.7} = exp(2.2123)$

= 9.1364

$k_{2} = 61 M^{-1}s^{-1}$

Thus, we can conclude that rate constant of this reaction is $61 M^{-1}s^{-1}$ .

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4 years ago

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Explanation:

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Your answer would be E. 470,000 J

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