The enzyme carbonic anhydrase catalyzes the following reaction: CO, + H,0 €→HCO; +H A. This reaction is important in the transport of carbon dioxide by red blood cells. Carbonic anhydrase has a molecular weight of ~27,000 g/mol and a turnover number (kcx) of approximately 1 X 10° per second. Assume you are given a solution that is saturated with Co, containing 4 ug of carbonic anhydrase. At what rate (in millimoles of CO, consumed per second) will this reaction proceed under optimal conditions? B. Assuming standard temperature and pressure, how much CO2 gas (in ml) will be consumed in 10 seconds?
The enzyme carbonic anhydrase catalyzes the following reaction: CO, + H,0 €→HCO; +H A. This reaction is important in the transport of carbon dioxide by red blood cells. Carbonic anhydrase has a molecular weight of ~27,000 g/mol and a turnover number (kcx) of approximately 1 X 10° per second. Assume you are given a solution that is saturated with Co, containing 4 ug of carbonic anhydrase. At what rate (in millimoles of CO, consumed per second) will this reaction proceed under optimal conditions? B. Assuming standard temperature and pressure, how much CO2 gas (in ml) will be consumed in 10 seconds?
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![# Carbonic Anhydrase Enzyme Reaction
## Description:
The enzyme carbonic anhydrase catalyzes the following reaction:
\[ \text{CO}_2 + \text{H}_2\text{O} \leftrightarrow \text{HCO}_3^- + \text{H}^+ \]
---
### Part A
This reaction is critical for the transport of carbon dioxide (CO₂) by red blood cells. The carbonic anhydrase enzyme has the following characteristics:
- **Molecular weight**: Approximately 27,000 g/mol
- **Turnover number (k_cat)**: Approximately 1 × 10⁶ per second
**Question:**
Given a solution saturated with CO₂ and containing 4 µg (micrograms) of carbonic anhydrase, at what rate (in millimoles of CO₂ consumed per second) will this reaction proceed under optimal conditions?
### Calculation Steps:
1. **Convert the mass of carbonic anhydrase to moles:**
\[
\text{Moles of carbonic anhydrase} = \frac{\text{mass (4 µg)}}{\text{molecular weight (27,000 g/mol)}}
\]
2. **Calculate the rate of reaction:**
\[
\text{Rate} = \text{moles of enzyme} \times k_{cat}
\]
---
### Part B
**Question:**
Assuming standard temperature and pressure (STP), how much CO₂ gas (in milliliters) will be consumed in 10 seconds?
### Calculation Steps:
1. **Use the rate from Part A to determine CO₂ consumption per second.**
2. **Convert the consumption rate to the volume, considering that 1 mole of gas at STP occupies 22.4 liters:**
\[
\text{Volume of CO₂ (at STP)} = \text{moles of CO₂} \times \text{molar volume at STP (22.4 L)}
\]
3. **Calculate the total volume for 10 seconds:**
\[
\text{Total Volume} = \text{Volume per second} \times 10
\]
By following these steps, one can determine the rate at which the carbonic anhydrase enzyme catalyzes the CO₂ reaction under optimal conditions and the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9e60ae64-4458-4b89-bb0e-7dd9dd5dc5fe%2F5dad9c77-853e-4caa-83a7-3a2eee5dd0d4%2Fl593ko6d_processed.png&w=3840&q=75)
Transcribed Image Text:# Carbonic Anhydrase Enzyme Reaction
## Description:
The enzyme carbonic anhydrase catalyzes the following reaction:
\[ \text{CO}_2 + \text{H}_2\text{O} \leftrightarrow \text{HCO}_3^- + \text{H}^+ \]
---
### Part A
This reaction is critical for the transport of carbon dioxide (CO₂) by red blood cells. The carbonic anhydrase enzyme has the following characteristics:
- **Molecular weight**: Approximately 27,000 g/mol
- **Turnover number (k_cat)**: Approximately 1 × 10⁶ per second
**Question:**
Given a solution saturated with CO₂ and containing 4 µg (micrograms) of carbonic anhydrase, at what rate (in millimoles of CO₂ consumed per second) will this reaction proceed under optimal conditions?
### Calculation Steps:
1. **Convert the mass of carbonic anhydrase to moles:**
\[
\text{Moles of carbonic anhydrase} = \frac{\text{mass (4 µg)}}{\text{molecular weight (27,000 g/mol)}}
\]
2. **Calculate the rate of reaction:**
\[
\text{Rate} = \text{moles of enzyme} \times k_{cat}
\]
---
### Part B
**Question:**
Assuming standard temperature and pressure (STP), how much CO₂ gas (in milliliters) will be consumed in 10 seconds?
### Calculation Steps:
1. **Use the rate from Part A to determine CO₂ consumption per second.**
2. **Convert the consumption rate to the volume, considering that 1 mole of gas at STP occupies 22.4 liters:**
\[
\text{Volume of CO₂ (at STP)} = \text{moles of CO₂} \times \text{molar volume at STP (22.4 L)}
\]
3. **Calculate the total volume for 10 seconds:**
\[
\text{Total Volume} = \text{Volume per second} \times 10
\]
By following these steps, one can determine the rate at which the carbonic anhydrase enzyme catalyzes the CO₂ reaction under optimal conditions and the
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