Posted by **Tasneem** on Saturday, April 7, 2012 at 10:14pm.

2. At 600 K the decomposition of gas ohase nitroethane (CH3CH2NO2) is first order with a rate constant of 1.9*10^-4 s^-1.

CH3CH2NO2 --> C2H4 + HNO2

a) Write out the differential and integrated rate laws for this reaction.

b) If a 10.0g sample of nitroethane is heated to 600K, what mass of nitroethane would be decomposed after 2.8 hours?

- Chemistry- Kinetics -
**DrBob222**, Saturday, April 7, 2012 at 10:40pm
I assume you can do a from your text or notes. Look it up if you have doubts.

b.

ln(No/N) = kt

No = 10.0g

N = unknown

k = 1.9E-4 sec^-1 (but this must be converted to hours or the time below into seconds).

t = 2.8 hours.

Solve for N to find how much remains, then subtract from 10.0 to find the amount decomposed.

- Chemistry- Kinetics -
**Tasneem**, Sunday, April 8, 2012 at 1:50am
Worked! Thank you! - Why is it ln(No/N) = kt though? The formula I have in my notes for first order reactions is ln(N1/No) = -kt

- Chemistry- Kinetics -
**ASMA**, Tuesday, April 9, 2013 at 3:23pm
BECAUSE THE MINUS SIGN WAS REMOVED IN THE EQUATION

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