CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Nernst Equation

For first ord...

Question

For first order parallel reaction $k_{1}$ and $k_{2}$ are $4$ and $2$ ${m i n}^{- 1}$ respectively at $300 K$ . If the activation energies for the formation of $B$ and $C$ are respectively $30, 000$ and $38, 314 j o u l e / m o l$ respectively. The temperature at which $B$ and $C$ will be obtained in equimolar ratio is:

A

757.48 K

No worries! We‘ve got your back. Try BYJU‘S free classes today!

B

378.74 K

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

C

600 K

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

none of these

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $378.74 K$
Two equations will be useful $A = A_{0} E^{- k t}$ and $\frac{k_{2}}{k_{1}} = e^{- \frac{E_{a}}{R} (\frac{T_{2} - T_{1}}{T_{1} T_{2}})}$ .
For the product B, $k = 2 e^{- \frac{30000}{8.314} (\frac{T_{2} - 300}{300 T_{2}})}$ .
And for the product C, $k = e^{- \frac{38314}{8.314} (\frac{T_{2} - 300}{300 T_{2}})}$ .
When equimolar mixture of B and C is formed,
$2 e^{- \frac{30000}{8.314} (\frac{T_{2} - 300}{300 T_{2}})} = e^{- \frac{38314}{8.314} (\frac{T_{2} - 300}{300 T_{2}})}$
Hence, $T_{2} = 378.74 K$ .

Suggest Corrections

thumbs-up

0

Similar questions

Q. For first order parallel reaction

k_{1}

k_{2}

4

2 m i n^{- 1}

respectively at

300 K

. The activation energies for the formation of

B

C

30, 000

38, 314 J / m o l

respectively. The temperature at which

B

C

will be obtained in equimolar ratio is:

Q. The activation energy for forward and backward reactions are

50 k J / m o l

40 k J / m o l

respectively. If

K_{1}

K_{2}

are the equilibrium constants of reaction at temperature

T_{1}

T_{2}

respectively and

T_{2} > T_{1}

Q. The ratio constants for

k_{1}

k_{2}

for two different reactions are

10^{16} e^{- 2000 T}

10^{15} e^{- 1000 / T}

respectively. Temperature at which

k_{1} = k_{2}

Q. A reactiontakes place in various steps. The rate constant for first, second, third and fifth steps are

k_{1}, k_{2}, k_{3}

k_{5}

respectively. The overall rate constant is given by:

k = \frac{k_{2}}{k_{3}} \times (\frac{k_{1}}{k_{5}})^{0.5}

If the activation energies are 40, 60, 50 and 10 kJ/mol respectively, the overall activation energy (kJ/mol) is:

Q. A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are

k_{1}, k_{2}, k_{3}

k_{5}

respectively. The overall rate constant is given by,

k = \frac{k_{2}}{k_{3}} [\frac{k_{1}}{k_{5}}]^{1 / 2}

If activation energy is

40, 60, 50

10 k J / m o l

respectively, the overall energy of activation

(k J / m o l)

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Nernst Equation

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Nernst Equation

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon