The following reaction was studied in the laboratory and the data shown in the table below was recorded at 25oC : A(g) + B(g)⟶C(g) + D(g) Trial A (mol/L) B (mol/L) Δ[C]/Δt (mol/L/s) 1 1.00 × 10−6 3.00 × 10−6 6.60 × 10−5 2 1.00 × 10−6 6.00 × 10−6 1.32 × 10−4 3 1.00 × 10−6 9.00 × 10−6 1.98 × 10−4 4 2.00 × 10−6 9.00 × 10−6 3.96 × 10−4 5 3.00 × 10−6 9.00 × 10−6 5.94 × 10−4 (a) Determine the order of reaction with respect to each reactant and the overall order. Show your working clearly. (b) Determine the value of the rate constant K. (c) Calculate the half-life of the reactant ‘A’ if initial concentration is 1 x 10-6 M. (d) Using this reaction as an example, explain the difference between stoichiometric coefficients, reaction order and molecularity.
The following reaction was studied in the laboratory and the data shown in the table below was recorded at 25oC :
A(g) + B(g)⟶C(g) + D(g)
|
Trial |
A (mol/L) |
B (mol/L) |
Δ[C]/Δt (mol/L/s) |
|
1 |
1.00 × 10−6 |
3.00 × 10−6 |
6.60 × 10−5 |
|
2 |
1.00 × 10−6 |
6.00 × 10−6 |
1.32 × 10−4 |
|
3 |
1.00 × 10−6 |
9.00 × 10−6 |
1.98 × 10−4 |
|
4 |
2.00 × 10−6 |
9.00 × 10−6 |
3.96 × 10−4 |
|
5 |
3.00 × 10−6 |
9.00 × 10−6 |
5.94 × 10−4 |
(a) Determine the order of reaction with respect to each reactant and the overall order. Show your working clearly.
(b) Determine the value of the rate constant K.
(c) Calculate the half-life of the reactant ‘A’ if initial concentration is 1 x 10-6 M.
(d) Using this reaction as an example, explain the difference between
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