Question

The rate constant for the decomposition of N2O5 increases from 1.52x10-5 s-1 at 25oC to 3.83x10-3...

The rate constant for the decomposition of N2O5 increases from 1.52x10-5 s-1 at 25oC to 3.83x10-3 s-1 at 45oC.

Calculate the activation energy for this reaction.

Homework Answers

Answer #1

thanks and hope you like the answer

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Values of the rate constant for the decomposition of N2O5 at four different temperatures are as...
Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows: T(K) k(s^-1) 658 2.14 x 10^5 673 3.23 x 10^5 688 4.81 x 10^5 703 7.03 x 10^5 Determine the activation energy of the decomposition reaction: _____kJ/mol Calculate the value of the rate constant at 300 K. _____s^-1
The rate constant for the decomposition of N2O5 is 7.78 × 10−7 at 273 K and...
The rate constant for the decomposition of N2O5 is 7.78 × 10−7 at 273 K and 3.46 × 10−5 at T2. If the activation energy is 1027 kJ/mol, what is the final temperature? 2 N2O5(g) → 4 NO2(g) + O2(g)
The rate constant for the first-order decomposition of N2O5 by the reaction 2 N2O5 (g) ...
The rate constant for the first-order decomposition of N2O5 by the reaction 2 N2O5 (g)  4 NO2(g) + O2(g) is k, = 3.38 x 10-5 s -1 at 25 C. What is the half-life of N2O5? What will be the partial pressure, initially 500 Torr, at ( a) 50 s; (b) 20 min, (c) 2 hr after initiation of the reaction?
In a series of experiments on the decomposition of dinitrogen pentoxide, N2O5, rate constants were determined...
In a series of experiments on the decomposition of dinitrogen pentoxide, N2O5, rate constants were determined at two different temperatures. At 35°C, the rate constant was 1.4×10-4/s; at 45°C, the rate constant was 5.0×10-4/s. (a) What is the activation energy for this reaction? (b) What is the value of the rate constant at 85°C?
if the decomposition of N2O5 has an activation energy of 103 kJ/mole and a frequency factor...
if the decomposition of N2O5 has an activation energy of 103 kJ/mole and a frequency factor of 4.3 *10^13 s^-1. what is the rate constant for this decomposition at 20°C?100°C?
The decomposition of N2O5 is first order reaction. N2O5(g) decomposes to yield NO2 (g) and O2(g)....
The decomposition of N2O5 is first order reaction. N2O5(g) decomposes to yield NO2 (g) and O2(g). At 48 deg C the rate constant for the reaction is 1.2x10^-5 s^-1. Calculate the partial pressure of NO2(g) produced from 1.0L of 0.700M N2O5 solution at 48 degC over a period of 22 hours if the gas is collected in a 10.0L container
If the rate constant increases from 0.40 M –1 s –1 at 25°C to 0.80 M...
If the rate constant increases from 0.40 M –1 s –1 at 25°C to 0.80 M –1 s –1 at 35°C, what is the activation energy in kJ/mol for this reaction?
The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the...
The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the following reaction: 2N2O5 (g) -> 4NO2 + O2 (g) Suppose that you start with .0175M of N2O5 (g) a.) What is the molarity of N2O5 that remains after 15 minutes (note: the rate constant is in seconds) b.) How many seconds will it take for the quantity of N2O5 to drop to .015M? c.) What is the half life of N2O5 at 70C?
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose...
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.10×10−2 mol of N2O5(g) in a volume of 1.8 L . How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol ?
The first-order rate constant for the decomposition of N2O5, given below, at 70°C is 6.82 10-3...
The first-order rate constant for the decomposition of N2O5, given below, at 70°C is 6.82 10-3 s-1. Suppose we start with 0.0550 mol of N2O5(g) in a volume of 3.5 L. 2 N2O5(g) → 4 NO2(g) + O2(g) (a) How many moles of N2O5 will remain after 3.0 min? mol (b) How many minutes will it take for the quantity of N2O5 to drop to 0.005 mol? min (c) What is the half-life of N2O5 at 70°C? min
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT