ADVANCED CHEMISTRY PROBLEM: CAN YOU SOLVE?

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

1 Answer

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  • 3 weeks ago

    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

    • Bobby_Thin
      Lv 7
      3 weeks 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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