Question
For a reaction 2A + B + 3C → D + 3E, the following data is obtained.
Exp. No. Concentration in mole per litre Initial rate of formation of D (torr s−1)
A B C
1 0.01 0.01 0.01 2.5 × 10−4
2 0.02 0.01 0.01 1.0 × 10−3
3 0.01 0.02 0.01 2.5 × 10−4
4 0.01 0.02 0.02 5.0 × 10−4
The order with respect to A, B and C are, respectively,
Options
Solution
r = K[A]x [B]y [C]z
Exp (1) ÷ Exp (2): $\frac{2.5 \times 10^{- 4}}{1.0 \times 10^{- 3}} = \frac{K(0.01)^{x}(0.01)^{y}(0.01)^{z}}{K(0.02)^{x}(0.01)^{y}(0.01)^{z}} \Rightarrow x = 2$
Exp (1) ÷ Exp (3): $\frac{2.5 \times 10^{- 4}}{2.5 \times 10^{- 4}} = \frac{K(0.01)^{x}(0.01)^{y}(0.01)^{z}}{K(0.01)^{x}(0.02)^{y}(0.01)^{z}} \Rightarrow y = 0$
Exp (3) ÷ Exp (4): $\frac{2.5 \times 10^{- 4}}{5.0 \times 10^{- 4}} = \frac{K(0.01)^{x}(0.02)^{y}(0.01)^{z}}{K(0.01)^{x}(0.02)^{y}(0.02)^{z}} \Rightarrow z = 1$
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