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Question
The following experimental rate data were obtained for a reaction carried out at 25°C:
\[\ce{A_{(g)} + B_{(g)} -> C_{(g)} + A_{(g)}}\]
| Initial [A(g)]/mol dm−3 | Initial [B(g)]/mol dm−3 | Initial rate/mol dm−3s−1 |
| 3.0 × 10−2 | 2.0 × 10−2 | 1.89 × 10−4 |
| 3.0 × 10−2 | 4.0 × 10−2 | 1.89 × 10−4 |
| 6.0 × 10−2 | 4.0 × 10−2 | 7.56 × 10−4 |
What are the orders with respect to A(g) and B(g)?
Options
Order with respect to A(g) Order with respect to B(g) Zero Second Order with respect to A(g) Order with respect to B(g) First Zero Order with respect to A(g) Order with respect to B(g) Second Zero Order with respect to A(g) Order with respect to B(g) Second First
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Solution
| Order with respect to A(g) | Order with respect to B(g) |
| Second | Zero |
Explanation:
Rate of reaction R = k[A]n [B]m
where n and m are the order of reaction w.r.t
A and B from the given table change A(g), keeping B(g) constant,
R1 = k[3 × 10−2]n [4 × 10−2]m = 1.89 × 10−4
R2 = k[6 × 10−2]n [4 × 10−2]m = 7.56 × 10−4
`(1/2)^"n" = 1/4` ⇒ n = 2
Change B(g), keeping A(g) constant,
R1 = k[3 × 10−2]n [2 × 10−2]m = 1.89 × 10−4
R2 = k[3 × 10−2]n [4 × 10−2]m = 1.89 × 10−4
`(1/2)^"m"` = 1 ⇒ m = 0
Therefore the order of reaction with respect to A(g) and B(g) will be second order and zero order, respectively.
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