Question

A certain reaction has an activation energy of 31.40 kJ/mol. At what Kelvin temperature will the...

A certain reaction has an activation energy of 31.40 kJ/mol. At what Kelvin temperature will the reaction proceed 6.50 times faster than it did at 293 K?

Use the Arrhenius equation

ln (k2/k1) = Ea/R [(1/T1)-(1/T2)]

Where R=8.3145 J/(molxK)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A certain reaction has an activation energy of 50.05 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 50.05 kJ/mol. At what Kelvin temperature will the reaction proceed 6.50 times faster than it did at 307 K?
A certain reaction has an activation energy of 65.39 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 65.39 kJ/mol. At what Kelvin temperature will the reaction proceed 3.50 times faster than it did at 337 K?
A certain reaction has an activation energy of 64.28 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 64.28 kJ/mol. At what Kelvin temperature will the reaction proceed 4.50 times faster than it did at 329 K?
A certain reaction has an activation energy of 53.03 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 53.03 kJ/mol. At what Kelvin temperature will the reaction proceed 7.00 times faster than it did at 365 K?
A certain reaction has an activation energy of 31.18 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 31.18 kJ/mol. At what Kelvin temperature will the reaction proceed 6.00 times faster than it did at 311 K?
A certain reaction has an activation energy of 47.88 kJ/mol. At what Kelvin temperature will the...
A certain reaction has an activation energy of 47.88 kJ/mol. At what Kelvin temperature will the reaction proceed 8.00 times faster than it did at 335K?
a.)A certain reaction has an activation energy of 25.10 kJ/mol. At what Kelvin temperature will the...
a.)A certain reaction has an activation energy of 25.10 kJ/mol. At what Kelvin temperature will the reaction proceed 7.00 times faster than it did at 289 K? b.A certain reaction has an enthalpy of ΔH = 39 kJ and an activation energy of Ea = 51 kJ. What is the activation energy of the reverse reaction? c.)At a given temperature, the elementary reaction A<=> B in the forward direction is the first order in A with a rate constant of...
The activation energy of a certain uncatalyzed reaction is 64 kJ/mol. In the presence of a...
The activation energy of a certain uncatalyzed reaction is 64 kJ/mol. In the presence of a catalyst, the Ea is 55 kJ/mol. How many times faster is the catalyzed than the uncatalyzed reaction at 400°C? Assume that the frequency factor remains the same.
1.) The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K the rate...
1.) The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K the rate constant is 6.1×10−8 s−1. What is the value of the rate constant at 860.0 K? ?=_____ s−1 2.) A certain reaction has an activation energy of 47.01 kJ/mol. At what Kelvin temperature will the reaction proceed 7.50 times faster than it did at 357 K? ____ K 3.) Consider this reaction data. A⟶products T (K) k (s–1) 275 0.383 875 0.659 If you were...
A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor of A1...
A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor of A1 = 2.80×1012 M−1s−1 . What is the rate constant, k, of this reaction at 30.0 ∘C ? I tried k = Ae^(-Ea/RT) but it's giving me 1.26E2 M^-1s^-1 which is wrong on my online homework, I did convert C to K and kJ/mol to J.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT