https://file.aiquickdraw.com/mathbot/file/1726855778556rpfm01hr.jpg

The problem asks for the mass of carbon dioxide consumed in the photosynthesis reaction, given that 4.38 g of water reacts.

First, let's recall the photosynthesis reaction:

\[
6 \text{CO}_2 + 6 \text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + 6 \text{O}_2
\]

This equation shows that 6 moles of carbon dioxide (CO₂) react with 6 moles of water (H₂O). Therefore, the reaction consumes equal molar amounts of CO₂ and H₂O.

### Step 1: Calculate the molar mass of water (H₂O)
The molar mass of H₂O is:
\[
M(\text{H}_2\text{O}) = 2(1.008) + 16.00 = 18.016 \, \text{g/mol}
\]

### Step 2: Calculate the number of moles of water (H₂O)
Given mass of water is 4.38 g. The number of moles of water is:
\[
\text{moles of H}_2\text{O} = \frac{\text{mass of H}_2\text{O}}{\text{molar mass of H}_2\text{O}} = \frac{4.38 \, \text{g}}{18.016 \, \text{g/mol}} \approx 0.2431 \, \text{mol}
\]

### Step 3: Use the stoichiometry of the reaction
From the balanced equation, 6 moles of H₂O react with 6 moles of CO₂, which implies a 1:1 molar ratio. So, the moles of CO₂ required are also 0.2431 mol.

### Step 4: Calculate the mass of carbon dioxide (CO₂)
The molar mass of CO₂ is:
\[
M(\text{CO}_2) = 12.01 + 2(16.00) = 44.01 \, \text{g/mol}
\]

Now, calculate the mass of CO₂:
\[
\text{mass of CO}_2 = \text{moles of CO}_2 \times M(\text{CO}_2) = 0.2431 \, \text{mol} \times 44.01 \, \text{g/mol} \approx 10.70 \, \text{g}
\]

So, the mass of carbon dioxide consumed is approximately **10.70 g**.

Would you like a detailed breakdown of any step or further clarification?

Here are some related questions to consider:
1. What is the role of carbon dioxide in photosynthesis?
2. How is stoichiometry used to balance chemical reactions?
3. What is the significance of molar ratios in chemical reactions?
4. How can you find the limiting reagent in a chemical reaction?
5. What are the products of photosynthesis, and how are they important to plants?

**Tip:** Always ensure that your final answer has the correct number of significant digits based on the given data.

What mass of carbon dioxide is consumed by the reaction of 4.38 g of water?

Learn how to calculate the mass of carbon dioxide consumed in a photosynthesis reaction when 4.38 g of water is used. This problem covers stoichiometry, molar mass calculations, and the law of conservation of mass. Suitable for high school chemistry students.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation