Respuesta :
The answer is: the mass of oxygen is 16.95 grams.
The overall balanced photosynthesis reaction:
6CO₂ + 6H₂O → C₆H₁₂O₆ + 6O₂.
m(C₆H₁₂O₆) = 15.90 g; mass of glucose.
n(C₆H₁₂O₆) = m(C₆H₁₂O₆) ÷ M(C₆H₁₂O₆).
n(C₆H₁₂O₆) = 15.9 g ÷ 180.18 g/mol.
n(C₆H₁₂O₆) = 0.088 mol; amount of glucose.
From chemical reaction: n(C₆H₁₂O₆) : n(O₂) = 1 : 6.
n(O₂) = 6 · 0.088 mol.
n(O₂) = 0.53 mol; amount of oxygen.
m(O₂) = 0.53 mol · 32.00 g/mol.
m(O₂) = 16.95 g; mass of oxygen.
Answer : The mass of [tex]O_2[/tex] forms are 16.94 grams.
Explanation : Given,
Mass of [tex]C_6H_{12}O_6[/tex] = 15.90 g
Molar mass of [tex]C_6H_{12}O_6[/tex] = 180.18 g/mole
Molar mass of [tex]O_2[/tex] = 32.00 g/mole
The balanced chemical reaction will be:
[tex]6CO_2(g)+6H_2O(g)\rightarrow C_6H_{12}O_6(s)+6O_2(g)[/tex]
First we have to calculate the moles of [tex]C_6H_{12}O_6[/tex]
[tex]\text{ Moles of }C_6H_{12}O_6=\frac{\text{ Mass of }C_6H_{12}O_6}{\text{ Molar mass of }C_6H_{12}O_6}=\frac{15.90g}{180.18g/mole}=0.08824moles[/tex]
Now we have to calculate the moles of [tex]O_2[/tex]
As, 1 mole of [tex]C_6H_{12}O_6[/tex] produced when 6 moles of oxygen produced
So, 0.08824 mole of [tex]C_6H_{12}O_6[/tex] produced when [tex]0.08824\times 6=0.5294[/tex] moles of oxygen produced
Now we have to calculate the mass of [tex]O_2[/tex]
[tex]\text{ Mass of }O_2=\text{ Moles of }O_2\times \text{ Molar mass of }O_2[/tex]
[tex]\text{ Mass of }O_2=(0.5294moles)\times (32.00g/mole)=16.94g[/tex]
Therefore, the mass of [tex]O_2[/tex] forms are 16.94 grams.
