For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is
[A] (mol L−1)
[B](mol L−1)
Initial rate
(mol L−1s−1)
0.05
0.05
0.045
0.10
0.05
0.090
0.20
0.10
0.72
(a)
Rate = k[A]2[B]2
(b)
Rate = k[A][B]
(c)
Rate = k[A]2[B]
(d)
Rate = k[A][B]2
For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is
|
[A] (mol L−1) |
[B](mol L−1) |
Initial rate (mol L−1s−1) |
|
0.05 |
0.05 |
0.045 |
|
0.10 |
0.05 |
0.090 |
|
0.20 |
0.10 |
0.72 |
(a)
Rate = k[A]2[B]2
(b)
Rate = k[A][B]
(c)
Rate = k[A]2[B]
(d)
Rate = k[A][B]2
Question ID - 52441 | SaraNextGen Top Answer
For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is
[A] (mol L−1)
[B](mol L−1)
Initial rate
(mol L−1s−1)
0.05
0.05
0.045
0.10
0.05
0.090
0.20
0.10
0.72
(a)
Rate = k[A]2[B]2
(b)
Rate = k[A][B]
(c)
Rate = k[A]2[B]
(d)
Rate = k[A][B]2
|
For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is
|
|||||||||||||||
|
(a) |
Rate = k[A]2[B]2 |
(b) |
Rate = k[A][B] |
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|
(c) |
Rate = k[A]2[B] |
(d) |
Rate = k[A][B]2 |
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2A + B → C
Rate = k[A]x[B]y
Exp-1, 0.045 = k[0.05]x [0.05]y …(i)
Exp-2, 0.090 = k[0.1]x[0.05]y …(ii)
Exp-3, 0.72 = k[0.2]x [0.1]y …(iii)
Divide equation (i) by equation (ii)
=
⇒x=1
Divide equation (i) by equation (iii)
= 
= 
⇒ y = 2
Rate law = k[A]1[B]2.