Question

5. The following reaction is a second order irreversible reaction: 2A + 3B2C i. Derive an expression for the rate of change in the concentration of A as a function of reaction time, initial concentrations and a second order rate constant. Solve this differential equation to yield an equation for fractional conversion of A as a function of time The rate constant is 0.02 L mmol min, and the initial concentrations of A, B, and C are 10 mmol/L, 10 mmol/L and 0 mmol/L, respectively. Draw a plot (neatly and accurately) of the concentrations of A, B, and C with time for the first 10 minutes of the reaction.

Answer 1

Anb 2A+33 2C Second order treoction) Given -A kc2A dNA A)V whene, NAs CAY A-akC X=1-CA CAO also dCA kch CA dca CA CA CAO 1 CAo CA CAO CA CA CAO (1-x)

CAO CAOlI-x : -x CAe kt X C kt CA kt -2 -3 2 Ca-Ce - C&-CR -3 -2 2 3CA-CA) Ce-CR) C Cao -3 (CA, - Ca) CAe 1+ktCA CB Cra-sCAt 2 x ( ktCA) Simlaly Ce CAoCA+Cco Cat kt C +kta For Ce CA nll Ca:O ka c021 mnmal min CA 10 +0.21 lo- 3t 27 HO.02x10X E) O.02X 102t I+O.02x Ot 21 Ca

CAneeC CACBT A ॐं +ो ८ टh कैं. ् Cc( ০০) = iO mmotlL
After 10 minutes

Ca = 3.3 mmol/L

Cb = 0 mmol/L

Cc = 5 mmol/L