Questions: Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the simple sugar glucose (C6H12O6) and oxygen gas (O2). What mass of oxygen gas is produced by the reaction of 8.5 g of carbon dioxide? Be sure your answer has the correct number of significant digits. g × 10

Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the simple sugar glucose (C6H12O6) and oxygen gas (O2).

What mass of oxygen gas is produced by the reaction of 8.5 g of carbon dioxide? Be sure your answer has the correct number of significant digits. g × 10

Transcript text: Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water $\left(\mathrm{H}_{2} \mathrm{O}\right)$ and carbon dioxide $\left(\mathrm{CO}_{2}\right)$ chemically react to form the simple sugar glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ and oxygen gas $\left(\mathrm{O}_{2}\right)$. What mass of oxygen gas is produced by the reaction of 8.5 g of carbon dioxide? Be sure your answer has the correct number of significant digits. $\square$ g $\square$ $\square \times 10$

Solution

Solution Steps

Step 1: Write the Balanced Chemical Equation

The balanced chemical equation for photosynthesis is:

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

This equation shows that 6 moles of carbon dioxide produce 6 moles of oxygen gas.

Step 2: Calculate Moles of Carbon Dioxide

First, we need to calculate the number of moles of carbon dioxide ($\text{CO}_2$) in 8.5 g. The molar mass of $\text{CO}_2$ is:

\[ \text{Molar mass of CO}_2 = 12.01 \, (\text{C}) + 2 \times 16.00 \, (\text{O}) = 44.01 \, \text{g/mol} \]

The number of moles of $\text{CO}_2$ is:

\[ \text{Moles of CO}_2 = \frac{8.5 \, \text{g}}{44.01 \, \text{g/mol}} = 0.1932 \, \text{mol} \]

Step 3: Calculate Moles of Oxygen Gas Produced

According to the balanced equation, 6 moles of $\text{CO}_2$ produce 6 moles of $\text{O}_2$. Therefore, the moles of $\text{O}_2$ produced are equal to the moles of $\text{CO}_2$:

\[ \text{Moles of O}_2 = 0.1932 \, \text{mol} \]

Step 4: Calculate Mass of Oxygen Gas Produced

The molar mass of $\text{O}_2$ is:

\[ \text{Molar mass of O}_2 = 2 \times 16.00 \, \text{g/mol} = 32.00 \, \text{g/mol} \]

The mass of $\text{O}_2$ produced is:

\[ \text{Mass of O}_2 = 0.1932 \, \text{mol} \times 32.00 \, \text{g/mol} = 6.1824 \, \text{g} \]