5. The above reaction was conducted at different initial concentrations of A and B and each time the initial rates of the reaction were determined (table 1) Table 1 Trial# 12 ● 3 [A] (M) 0.01 0.01 0.02 [B] (M) 181 (M) 0.02 0.04 0.01 The overall rate of the reaction = k [A]m [B]" Using the information on the table above explain: eta from which traits did you use and why? a) Is the reaction rate dependent on the concentration of A? the reaction By what factor the concentration of A changed? Overall rate (mol/sec) 0.001 0.004 0.002 0.002 . By what factor the overall reaction rate changed? • Is the reaction O-order with respect to A/is m =0? If not explain why? ils did you use? b) Is the reaction rate dependent on the concentration of B? down rate of the reaction= . By what factor the concentration of B changed? ● what factor the overall reaction rate changed? • Is the reaction 0-order with respect to B/is n = 0? If not explain why?

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### Determining Reaction Order Based on Experimental Data

The experiment described investigated the effect of varying initial concentrations of reactants A and B on the initial rate of a reaction. The data is summarized in the table below:

#### Table 1 - Experimental Data

| Trial # | [A] (M) | [B] (M) | Overall Rate (mol/sec) |
| ------- | ------- | ------- | --------------------- |
| 1       | 0.01    | 0.02    | 0.001                 |
| 2       | 0.01    | 0.04    | 0.004                 |
| 3       | 0.02    | 0.01    | 0.002                 |

The overall rate of the reaction can be described by the rate equation:
\[ \text{Rate} = k [A]^m [B]^n \]

Using the information from Table 1, we can answer the following questions:

#### a) Dependency of the Reaction Rate on the Concentration of A

1. **Is the reaction rate dependent on the concentration of A?**
   - **Explanation:** To determine if the reaction rate depends on the concentration of A, we compare Trials 1 and 3, where the concentration of B is kept constant at 0.01 M.
   
2. **By what factor the concentration of A changed?**
   - In comparing Trials 1 and 3: 
     \[ \text{[A]} \text{ (trial 3)} = 0.02 \; \text{M}, \; \text{[A]} \text{ (trial 1)} = 0.01 \; \text{M} \rightarrow \text{Factor change} = \frac{0.02}{0.01} = 2 \]
   
3. **By what factor the overall reaction rate changed?**
   - The reaction rate changes from 0.001 mol/sec (Trial 1) to 0.002 mol/sec (Trial 3):
     \[ \text{Rate} \text{ (trial 3)} = 0.002 \; \text{mol/sec}, \; \text{Rate} \text{ (trial 1)} = 0.001 \; \text{mol/sec} \rightarrow \text{Factor change} = \frac{0.002}{0
Transcribed Image Text:### Determining Reaction Order Based on Experimental Data The experiment described investigated the effect of varying initial concentrations of reactants A and B on the initial rate of a reaction. The data is summarized in the table below: #### Table 1 - Experimental Data | Trial # | [A] (M) | [B] (M) | Overall Rate (mol/sec) | | ------- | ------- | ------- | --------------------- | | 1 | 0.01 | 0.02 | 0.001 | | 2 | 0.01 | 0.04 | 0.004 | | 3 | 0.02 | 0.01 | 0.002 | The overall rate of the reaction can be described by the rate equation: \[ \text{Rate} = k [A]^m [B]^n \] Using the information from Table 1, we can answer the following questions: #### a) Dependency of the Reaction Rate on the Concentration of A 1. **Is the reaction rate dependent on the concentration of A?** - **Explanation:** To determine if the reaction rate depends on the concentration of A, we compare Trials 1 and 3, where the concentration of B is kept constant at 0.01 M. 2. **By what factor the concentration of A changed?** - In comparing Trials 1 and 3: \[ \text{[A]} \text{ (trial 3)} = 0.02 \; \text{M}, \; \text{[A]} \text{ (trial 1)} = 0.01 \; \text{M} \rightarrow \text{Factor change} = \frac{0.02}{0.01} = 2 \] 3. **By what factor the overall reaction rate changed?** - The reaction rate changes from 0.001 mol/sec (Trial 1) to 0.002 mol/sec (Trial 3): \[ \text{Rate} \text{ (trial 3)} = 0.002 \; \text{mol/sec}, \; \text{Rate} \text{ (trial 1)} = 0.001 \; \text{mol/sec} \rightarrow \text{Factor change} = \frac{0.002}{0
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