Posted by **selly** on Friday, January 11, 2013 at 10:26am.

The rate constants for a first order decay reaction are found to be:

k287.3∘C=1 x 10−4 s−1

k327.4∘C=19.2 x 10−4 s−1

(a) Determine the value, in s-1 of k250∘C

(b) How long will it take, at 350 ∘C, for the reactant to decay to 1% of its original concentration? Express your answer in seconds.

- Chemistry -
**Chemgam**, Friday, January 11, 2013 at 10:36am
a)4.27*10^-6

b)536.7

- Chemistry -
**Anonymous**, Friday, January 11, 2013 at 2:29pm
aja MITx FINAL EXAM

## Answer This Question

## Related Questions

- chemistry - The rate constants for a first order decay reaction are found to be...
- Chemistry - Given the following half-reactions and associated standard reduction...
- Math - Finding the Equation - If.... f(x) = x + 2 and g(x) = −x^2 + 2x &#...
- Math (Trigonometry [Polar Form]) - Let z be a complex number such that z = 2(cos...
- Chemistry - Calculate value of Ksp for Ca(OH)2 (ΔG∘f(Ca2+)=-553.6 ...
- Chemistry - Free-energy change, ΔG∘, is related to cell potential, E...
- chemistry - kinetics - Understanding the high-temperature behavior of nitrogen ...
- Chemistry - H6P6: Urbium Oxide First Part of the Question: Urbium (Ur) is an ...
- Chem - Calculate the standard cell potential given the following standard ...
- chemistry - Urbium (Ur) is an upscale element found in big cities. Its oxide (...

More Related Questions