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प्रश्न
For the non-stoichiometric reaction, \[\ce{2A + B -> C + D}\], the following kinetic data were obtained in three separate experiments, all at 298 K.
| Initial concentration (A) |
Initial concentration (B) |
Initial rate of formation of C (mol L−1 s−1) |
| 0.1 M | 0.1 M | 1.2 × 10−3 |
| 0.1 M | 0.2 M | 1.2 × 10−3 |
| 0.2 M | 0.1 M | 2.4 × 10−3 |
The rate law for the formation of C is:
विकल्प
`(dc)/(dt) = k[A][B]`
`(dc)/(dt) = k[A]^2[B]`
`(dc)/(dt) = k[A][B]^2`
`(dc)/(dt) = k[A]`
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उत्तर
`bb((dc)/(dt) = k[A])`
Explanation:
The rate law expression is k[A]x[B]y
∴ `("d"["C"])/"dt"` = k[A]x[B]y
Substituting the given values in above equation for three separate experiments we get,
1.2 × 10−3 = k[0.1]x[0.1]y ...(i)
1.2 × 10−3 = k[0.1]x[0.2]y ...(ii)
2.4 × 10−3 = k[0.2]x[0.1]y ...(iii)
Dividing equation (i) by (ii)
`(1.2 xx 10^-3)/(1.2 xx 10^-3) = (k[0.1]^x [0.1]y)/(k[0.1]^x [0.2]^y)`
1 = `[1/2]^y` ...(∴ y = 0)
Now Dividing equation (i) by (iii)
`(1.2 xx 20^-3)/(2.4 xx 10^-3) = (k[0.1]^x [0.1]^y)/(k[0.2]^x [0.1]^y)`
`[1/2]^1 = [1/2]^x`
x = 1
