The reaction is thought to be a multi-step reaction, and the following partial mechanism showing the possible slow step has been proposed. Does this mechanism agree with the rate law? And why or why not? Ni(CO)4 Ni(CO); + CO (slow)

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please see attached blue checked question. The following is the rate of reaction in order to answer the question:

Rate = K X [Ni(CO)4 ]1

## Reaction Kinetics Study: Ni(CO)₄ Decomposition

### Reaction Overview
The reaction under study is the decomposition of nickel tetracarbonyl:
\[ \text{Ni(CO)}_4 (g) \rightarrow \text{Ni} (s) + 4 \text{CO} (g) \]

### Rate Law and Reactant Concentration

#### Experimental Data: Effect of Time on [Ni(CO)₄]
The kinetics of this reaction were studied at 50.9°C. The following data were obtained by monitoring the concentration of \(\text{Ni(CO)}_4\) over time:

| Time (sec) | \([\text{Ni(CO)}_4] \, (M)\) |
|------------|-----------------------------|
| 1.0        | 0.45                        |
| 2.0        | 0.35844                     |
| 4.0        | 0.221683                    |
| 6.0        | 0.109202                    |
| 10.0       | 0.053799                    |
| 15.0       | 0.013056                    |
| 20.0       | 0.002224                    |

**Determining Reaction Order:**
- What is the order of the reaction with respect to \(\text{Ni(CO)}_4\)?

**Half-Life Calculation:**
- What is the half-life of the reaction, in minutes, at 50.9°C?

### Temperature Effect on Reaction Kinetics

#### Experimental Data: Rate Constants at Various Temperatures
This same reaction's kinetics were also studied at five different temperatures. The rate constant (\(k\)) was measured for each temperature:

| Temperature (°C) | \(k\) (sec\(^{-1}\)) |
|------------------|---------------------|
| 47.3             | 0.263               |
| 50.9             | 0.354               |
| 55.0             | 0.606               |
| 60.0             | 1.022               |
| 66.0             | 1.873               |

**Activation Energy Calculation:**
- Using the Arrhenius equation and the data provided, calculate the activation energy (in kJ/mol) for this reaction. \(R = 8.314 \, \text{J
Transcribed Image Text:## Reaction Kinetics Study: Ni(CO)₄ Decomposition ### Reaction Overview The reaction under study is the decomposition of nickel tetracarbonyl: \[ \text{Ni(CO)}_4 (g) \rightarrow \text{Ni} (s) + 4 \text{CO} (g) \] ### Rate Law and Reactant Concentration #### Experimental Data: Effect of Time on [Ni(CO)₄] The kinetics of this reaction were studied at 50.9°C. The following data were obtained by monitoring the concentration of \(\text{Ni(CO)}_4\) over time: | Time (sec) | \([\text{Ni(CO)}_4] \, (M)\) | |------------|-----------------------------| | 1.0 | 0.45 | | 2.0 | 0.35844 | | 4.0 | 0.221683 | | 6.0 | 0.109202 | | 10.0 | 0.053799 | | 15.0 | 0.013056 | | 20.0 | 0.002224 | **Determining Reaction Order:** - What is the order of the reaction with respect to \(\text{Ni(CO)}_4\)? **Half-Life Calculation:** - What is the half-life of the reaction, in minutes, at 50.9°C? ### Temperature Effect on Reaction Kinetics #### Experimental Data: Rate Constants at Various Temperatures This same reaction's kinetics were also studied at five different temperatures. The rate constant (\(k\)) was measured for each temperature: | Temperature (°C) | \(k\) (sec\(^{-1}\)) | |------------------|---------------------| | 47.3 | 0.263 | | 50.9 | 0.354 | | 55.0 | 0.606 | | 60.0 | 1.022 | | 66.0 | 1.873 | **Activation Energy Calculation:** - Using the Arrhenius equation and the data provided, calculate the activation energy (in kJ/mol) for this reaction. \(R = 8.314 \, \text{J
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