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The following results have been obtained during the kinetic studies of the reaction: P + 2Q \(\rightarrow\) R + 2SExp.Initial P(mol/L)Initial Q(mol/L)Init. Rate of Formation of R (M min-1)10.100.103.0 x 10-420.300.309.0 x 10-430.100.303.0 x 10-440.400.406.0 x 10-4Determine the rate law expression for the reaction. |
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Answer» let the rate law expression be Rate = k [P]x [Q]y from the table we know that Rate 1 = 3.0 x 10-4 = k (0.10)x (0.10)y Rate 2 = 9.0 x 10-4 = k (0.30)x (0.30)y Rate 3 = 3.0 x 10-4 = k (0.10)x (0.30)y \(\frac{Rate\,1}{Rate\,3}\)= (\(\frac{1}{3}\))y or 1 = (\(\frac{1}{3}\))y So y = 0 \(\frac{Rate\,2}{Rate\,3}\)= (3)x or 3 = (3)x So x = 1 Rate = k [P] |
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