ADVANCED CHEMISTRY PROBLEM: CAN YOU SOLVE?

Question

Q) How many liters of CO2(g), measured at 24.5oC and 748 mmHg, are produced as a 10.0 g sample of CH3COCH2COOH decomposes for 575 min? (Ignore the aqueous solubility of CO2(g).) Ignore the aqueous solubility of CO2. The half life of the CH3COCH2COOH  is 144 mins

Update:

Btw  CH3COCH2COOH is first order decomposition

Answer 1

CH3COCH2COOH (aq) → CH3COCH3 (aq) + CO2 (g)

This first-order decomposition has a half-life of 144 min. 

Use the rate constant and the first-order concentration-time equation to determine the reactant concentration at the given time.

V = 2.28 L

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• Bobby_Thin

  Lv 7

  8 months agoReport

  read up on first order kinetics and half life . Use the rate constant and the first-order concentration-time equation to determine the reactant concentration at the given time.
  

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