Posted by **Kyo** on Friday, November 19, 2010 at 3:07am.

1. The reaction,

CO(CH2COOH)2 CO(CH3)2 + 2CO2,

follows first-order kinetics and has an activation energy of 96.6 kJ mol-1. At 293 K, k = 0.133 s-1. Find the temperature (in K) at which half-live will be 0.00692 min? Round your answer to 3 significant figures.

Okay so i tried converting the half-life back to k by multiplying it by 60 (convert min to s) and than multiplying it by .693 (1st order half life eq)

and than i plugged it into ln(k1/k2) = Ea/R (t1-t2/t1*t2) and got 299K but the answer is 313...

2. The reaction,

H2 + I2 2HI,

has a rate constant k = 0.00110 L mol-1 s-1 at 683 K and k = 0.00275 L mol-1 s-1 at 700 K. What is the rate constant for the reaction at 443 °C? Round your answer to 3 significant figures.

So for this problem i tried finding Ea by using the first set of k and temperatures...and got 214.246 kj/mol but i don't know what to do next

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