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?

Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
icon
Concept explainers
Question

Need help with B not A

# 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
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
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 1 images

Blurred answer
Knowledge Booster
Ionic Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY