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tester [92]
1 year ago
15

C6H12 + 9 O2 –> 6 CO2 + 6 H2O

Chemistry
1 answer:
baherus [9]1 year ago
6 0

5.76 g of O_2 are consumed when C_6H_1_2 is burned to yield 5.3 grams of CO_2.

<h3>What is a mole?</h3>

A mole is defined as 6.02214076 × 10^{23} of some chemical unit, be it atoms, molecules, ions, or others.

Calculating moles of CO_2

Number of mole of CO_2 = \frac{\;Given \;mass}{\;Molar \;mass}

\frac{\;Given \;mass}{\;Molar \;mass} = \frac{5.3g}{44 g/mol} = 0.12 mol

As is clear from the reaction stoichiometry, 9 moles of O_26 moles of CO_2.

Calculating the number of moles of CO_2

\frac{0.12 X 9}{6} = 0.18 mol

Mass of O_2 =5.76 g

Hence, 5.76 g of O_2 are consumed when C_6H_1_2 yield 5.3 grams of CO_2.

Learn more about mole here:

brainly.com/question/26416088

#SPJ1

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3 years ago
How many grams of NH3 can be produced from 2.51 mil of N2 and excess H2 ?
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85.34g of NH3

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

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Step 2:

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From the balanced equation above,

1 mole of N2 reacted to produce 2 moles of NH3.

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2 years ago
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