Nitrification of water is a biological process for removing ammonia from wastewater as ammonium: NH4 (aq) + 2 02 (g) --> NO31 (aq) + 2 H* (aq) + H2O (1) The first-order rate constant is given as: k = 0.47eº.095(T – 0.15°C) where k is in day1 and T is in degrees Celsius. a. If the initial concentration of NH3 is 4.0 mol/m³, how long will it take to reduce the concentration to 0.80 mol/m³ in the spring (T = 20°C) b. Assuming the same amounts in part a, how long will it take to reduce the concentration in the winter (T = 10°C) c. Using your answer in part a, what is the rate of 02 consumption?
Nitrification of water is a biological process for removing ammonia from wastewater as ammonium: NH4 (aq) + 2 02 (g) --> NO31 (aq) + 2 H* (aq) + H2O (1) The first-order rate constant is given as: k = 0.47eº.095(T – 0.15°C) where k is in day1 and T is in degrees Celsius. a. If the initial concentration of NH3 is 4.0 mol/m³, how long will it take to reduce the concentration to 0.80 mol/m³ in the spring (T = 20°C) b. Assuming the same amounts in part a, how long will it take to reduce the concentration in the winter (T = 10°C) c. Using your answer in part a, what is the rate of 02 consumption?
Chemistry
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Chapter1: Chemical Foundations
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![**Nitrification of Water: A Biological Process**
Nitrification is a biological process used to remove ammonia from wastewater by converting it into ammonium. The chemical reaction involved is:
\[ \text{NH}_4^+ \, (\text{aq}) + 2 \, \text{O}_2 \, (\text{g}) \rightarrow \text{NO}_3^- \, (\text{aq}) + 2 \, \text{H}^+ \, (\text{aq}) + \text{H}_2\text{O} \, (\text{l}) \]
The rate of this process is described by a first-order rate constant:
\[ k = 0.47e^{0.095(T - 0.15^\circ \text{C})} \]
where \( k \) is given in day\(^{-1}\) and \( T \) is the temperature in degrees Celsius.
### Problems:
a. Given an initial concentration of NH\(_3\) at 4.0 mol/m\(^3\), determine how long it will take to reduce this concentration to 0.80 mol/m\(^3\) during spring (\( T = 20^\circ \text{C} \)).
b. Using the same initial and target concentrations, calculate the time required to achieve this reduction during winter (\( T = 10^\circ \text{C} \)).
c. Referencing the solution to part a, determine the rate of O\(_2\) consumption.
> Note: Parts of the text in the original image are obscured.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1da2b7e6-ff1f-4d03-afb3-6b710fedc971%2F49011155-1071-4344-9a14-eaccc7653cc7%2Fxbkba5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Nitrification of Water: A Biological Process**
Nitrification is a biological process used to remove ammonia from wastewater by converting it into ammonium. The chemical reaction involved is:
\[ \text{NH}_4^+ \, (\text{aq}) + 2 \, \text{O}_2 \, (\text{g}) \rightarrow \text{NO}_3^- \, (\text{aq}) + 2 \, \text{H}^+ \, (\text{aq}) + \text{H}_2\text{O} \, (\text{l}) \]
The rate of this process is described by a first-order rate constant:
\[ k = 0.47e^{0.095(T - 0.15^\circ \text{C})} \]
where \( k \) is given in day\(^{-1}\) and \( T \) is the temperature in degrees Celsius.
### Problems:
a. Given an initial concentration of NH\(_3\) at 4.0 mol/m\(^3\), determine how long it will take to reduce this concentration to 0.80 mol/m\(^3\) during spring (\( T = 20^\circ \text{C} \)).
b. Using the same initial and target concentrations, calculate the time required to achieve this reduction during winter (\( T = 10^\circ \text{C} \)).
c. Referencing the solution to part a, determine the rate of O\(_2\) consumption.
> Note: Parts of the text in the original image are obscured.
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