If a new reaction was run leaving [N] the same, but beginning (time = 0) with [M] = 0.204 M, A(545nm) = 0.981. After 30 seconds, A (545 nm) is 0.807. What is the order of the reaction with respect to [M] ?
If a new reaction was run leaving [N] the same, but beginning (time = 0) with [M] = 0.204 M, A(545nm) = 0.981. After 30 seconds, A (545 nm) is 0.807. What is the order of the reaction with respect to [M] ?
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![**Determining the Order of a Reaction with Respect to [M]**
*Problem Statement:*
If a new reaction was run leaving [N] the same, but beginning (time = 0) with [M] = 0.204 M, A(545nm) = 0.981. After 30 seconds, A(545 nm) is 0.807. What is the order of the reaction with respect to [M]?
*Explanation:*
We are given initial conditions with specific absorbance values, measured at a wavelength of 545 nm. With these data points, the goal is to determine the reaction order with respect to the concentration of M, identified as [M].
- At time t = 0, the concentration of M is 0.204 M and the absorbance A(545nm) is 0.981.
- After 30 seconds, the absorbance at 545 nm changes to 0.807.
To determine the order of the reaction with respect to [M], we need to examine how the concentration of [M] affects the rate of the reaction. Using the change in absorbance over time at a specific wavelength, we can apply various rate laws and observe which one fits the data.
**Steps to Determine the Order:**
1. **Zero-Order Reaction:**
- For a zero-order reaction, the rate of reaction is constant.
- [M] would decrease linearly with time.
2. **First-Order Reaction:**
- The rate of reaction depends linearly on the concentration of [M].
- The plot of ln[M] versus time should be linear.
3. **Second-Order Reaction:**
- The rate is proportional to the square of the concentration of [M].
- The plot of 1/[M] versus time should be linear.
Considering the given absorbance values, we can relate them to concentration changes using Beer's Law (A = εlc, where A is absorbance, ε is molar absorptivity, l is path length, and c is concentration). Since l and ε remain constant, any change in absorbance can be directly related to the change in concentration.
Once you have these plots, identify the linear relationship among zero, first, or second-order reactions. The order in which the graphical representation (linear plot) fits best will indicate the order of reaction concerning [M].
This step-by-step process is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1dedc2f0-34a2-4f6a-9bbc-fab867b2dfd0%2F6a89ef10-f8de-43e1-9689-6fb2ee569fd9%2Fmaj2ipj.png&w=3840&q=75)
Transcribed Image Text:**Determining the Order of a Reaction with Respect to [M]**
*Problem Statement:*
If a new reaction was run leaving [N] the same, but beginning (time = 0) with [M] = 0.204 M, A(545nm) = 0.981. After 30 seconds, A(545 nm) is 0.807. What is the order of the reaction with respect to [M]?
*Explanation:*
We are given initial conditions with specific absorbance values, measured at a wavelength of 545 nm. With these data points, the goal is to determine the reaction order with respect to the concentration of M, identified as [M].
- At time t = 0, the concentration of M is 0.204 M and the absorbance A(545nm) is 0.981.
- After 30 seconds, the absorbance at 545 nm changes to 0.807.
To determine the order of the reaction with respect to [M], we need to examine how the concentration of [M] affects the rate of the reaction. Using the change in absorbance over time at a specific wavelength, we can apply various rate laws and observe which one fits the data.
**Steps to Determine the Order:**
1. **Zero-Order Reaction:**
- For a zero-order reaction, the rate of reaction is constant.
- [M] would decrease linearly with time.
2. **First-Order Reaction:**
- The rate of reaction depends linearly on the concentration of [M].
- The plot of ln[M] versus time should be linear.
3. **Second-Order Reaction:**
- The rate is proportional to the square of the concentration of [M].
- The plot of 1/[M] versus time should be linear.
Considering the given absorbance values, we can relate them to concentration changes using Beer's Law (A = εlc, where A is absorbance, ε is molar absorptivity, l is path length, and c is concentration). Since l and ε remain constant, any change in absorbance can be directly related to the change in concentration.
Once you have these plots, identify the linear relationship among zero, first, or second-order reactions. The order in which the graphical representation (linear plot) fits best will indicate the order of reaction concerning [M].
This step-by-step process is
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