I have some trouble finding the correct solution for the following problem:The eliminaion of carbon dioxide from pyruvate ions by a decarboxylase enzyme was monitored by measuring the partial pressure of the gas as it was formed in a 250 mLflask at 20°C. In one experiment the partial pressure increased from zer o to 100 Pa in 522 s in a first order reaction when the initial concentration of pyruvate ions in 100 mL of solution was 3.32 mmol / L. What is the rate constant of the reaction?
____________________________________________________________________________________________________This is what I attempted:
strategy: use the 1st order integrated rate law (with partial pressures) and consider the consumption of pyruvate ions.
integrated first order rate law:
ln(p-final) = ln(p-initial) - ktp initial
p = nRT / V = 0.0315 bar
where V = 0.25l
and n = c*V = 3.23 mmol/l *0.1 l = 3.23*10^(-4)p final
p final = p-initial - delta p = 0.0315 bar - 0.001 bar = 0.0305 bar rate constant k
k' = -k = -6.2 * 10^(-5) 1/s
k = 6.2 *10^(-5) 1/s
the correct answer, however, is 4.2* 10^(-5) 1/s
Does anyone see what I am doing wrong?
Thanks so much for any help/hints/suggestions!