Simple Rate Equations, Orders of Reaction & Rate Constants
1. This question has 4 part(s).
1.1. The reaction
A + 2B + 2C → D + 2E
was studied. The following initial rates data were collected at 298 K in Table 4.1.
Table 4.1
experiment | [A] / mol dm-3 | [B] / mol dm-3 | [C] / mol dm-3 | initial rate / mol dm-3 s-1 |
|---|---|---|---|---|
1 | 0.040 | 0.120 | 0.050 | 1.20 x 10-5 |
2 | 0.060 | 0.120 | 0.050 | 1.80 x 10-5 |
3 | 0.040 | 0.060 | 0.050 | 3.00 x 10-6 |
4 | 0.080 | 0.060 | 0.150 | 6.00 x 10-6 |
Use the data in Table 4.1 to deduce the order of reaction with respect to A, B, and C.
Show your mathematical reasoning.
1.2. (i) Write the rate equation for the reaction.
[1]
(ii) Calculate the value of the rate constant, k, for Experiment 1. Include the units for k.
k = .................... units = ...................
[3]
1.3. Suggest a two-step mechanism for this reaction where the first step is the rate-determining step.
1.4. The reaction between I− and S2O82− is slow due to high activation energy.
S2O82− (aq) + 2e− ⇌ 2SO42− (aq) Eθ=+2.01 V
Fe3+ (aq) + e−⇌ Fe2+ (aq) Eθ=+0.77 V
I2 (aq) + 2e− ⇌ 2I− (aq) Eθ=+0.54 V
Explain, using the Eθ values provided, why Fe2+ ions are an effective catalyst for this reaction.
Ai এর মাধ্যমে
১০ লক্ষ+ প্রশ্ন ডাটাবেজ
প্র্যাকটিস এর মাধ্যমে নিজেকে তৈরি করে ফেলো
উত্তর দিবে তোমার বই থেকে ও তোমার মত করে।
সারা দেশের শিক্ষার্থীদের মধ্যে নিজের অবস্থান যাচাই
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