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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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Find the percentage of mass in each of the element Ca ( HCO3)2 (Ca= 40, H = 1, O = 16, C= 35)​
Alex787 [66]

Answer:

% Ca = 24.69%

% H = 1.2%

% C = 14.8%

% O = 59.25%

Explanation:

The percentage by mass of each element can be calculated by dividing the mass of each element in the compound by the molar mass of the compound.

Molar mass of Ca(HCO3)2

Where; (Ca= 40, H = 1, O = 16, C= 12)

= 40 + {1 + 12 + 16(3)}2

= 40 + {13 + 48}2

= 40 + {61}2

= 40 + 122

= 162g/mol

- % mass of Ca = 40/162 × 100

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- % mass of H = 2/162 × 100

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- % mass of C = 24/162 × 100

= 0.148 × 100

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- % mass of O = 96/162 × 100

= 0.5925 × 100

= 59.25%

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Bananas Foster is an example of a dessert that is flambéed. A Bananas Foster label states the accepted number of Calories to be
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Answer:

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Measured value for the number of calories in a Bananas Foster: 318 calories

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