Answer:
[tex]\boxed{\text{136 g}}[/tex]
Explanation:
We will need an equation with masses and molar masses, so let’s gather all the information in one place.
M_r: 44.01 180.16
6CO₂ + 6H₂O ⟶ C₆H₁₂O₆ + 6O₂
m/g: 200
1. Moles of CO₂
[tex]\text{Moles of CO}_{2} = \text{200 g CO}_{2} \times \dfrac{\text{1 mol CO}_{2}}{\text{ 44.01g CO}_{2}} = \text{4.54 mol CO}_{2}[/tex]
2. Moles of C₆H₁₂O₆
The molar ratio is 1 mol C₆H₁₂O₆:6 mol CO₂
[tex]\text{Moles of C$_{6}$H$_{12}$O}_{6} =\text{4.54 mol CO}_{2} \times \dfrac{\text{1 mol C$_{6}$H$_{12}$O}_{6}}{\text{6 mol CO}_{2}} = \text{0.757 mol C$_{6}$H$_{12}$O}_{6}[/tex]
3. Mass of C₆H₁₂O₆
[tex]\text{Mass of C$_{6}$H$_{12}$O}_{6} = \text{0.757 mol C$_{6}$H$_{12}$O}_{6} \times \dfrac{\text{180.16 g C$_{6}$H$_{12}$O}_{6}}{\text{1 mol C$_{6}$H$_{12}$O}_{6}} =\textbf{136 g C$_{6}$H$_{12}$O}_{6}\\\\\text{The plants can create }\boxed{\textbf{136 g C$_{6}$H$_{12}$O}_{6}}[/tex]
