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SVETLANKA909090 [29]
3 years ago
13

What mass of oxygen (O2) forms in a reaction that forms 15.90 g C6H12O6? (Molar mass of O2 = 32.00 g/mol; molar mass of C6H12O6

= 180.18 g/mol) 15.90 g C6H12O6 = g O2
Chemistry
2 answers:
Dafna11 [192]3 years ago
5 0

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.

slamgirl [31]3 years ago
3 0

Answer : The mass of O_2 forms are 16.94 grams.

Explanation : Given,

Mass of C_6H_{12}O_6 = 15.90 g

Molar mass of C_6H_{12}O_6 = 180.18 g/mole

Molar mass of O_2 = 32.00 g/mole

The balanced chemical reaction will be:

6CO_2(g)+6H_2O(g)\rightarrow C_6H_{12}O_6(s)+6O_2(g)

First we have to calculate the moles of C_6H_{12}O_6

\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

Now we have to calculate the moles of O_2

As, 1 mole of C_6H_{12}O_6 produced when 6 moles of oxygen produced

So, 0.08824 mole of C_6H_{12}O_6 produced when 0.08824\times 6=0.5294 moles of oxygen produced

Now we have to calculate the mass of O_2

\text{ Mass of }O_2=\text{ Moles of }O_2\times \text{ Molar mass of }O_2

\text{ Mass of }O_2=(0.5294moles)\times (32.00g/mole)=16.94g

Therefore, the mass of O_2 forms are 16.94 grams.

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