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brilliants [131]
2 years ago
8

Find the empirical formula of the compound which contains 67.6% Hg, 10.8% S, and 21.6% O.

Chemistry
1 answer:
WINSTONCH [101]2 years ago
7 0

Explanation:

Divide 67.6% by 201 of mercury

Divide 10.8% by 32 of sulfur

Divide 21.6% by 16 of oxygen

Then divide number by itself .

Example : Divide 2.97 by both sulfer moles and oxygen moles . Multiply by 2 to get whole number

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Calculate the mass in grams of carbon dioxide produced from 11.2 g of octane (C8H18) in the reaction above.
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Answer:

34.6g

Explanation:

Given parameters:

Mass of Octane  = 11.2g

  Reaction expression;

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Mass of octane = 11.2g

Unknown:

Mass of carbon dioxide produced  = ?

Solution:

From the balanced reaction equation;

         2 mole of octane produced 16 moles of carbon dioxide

From the given specie, let us find the number of moles;

    Number of moles  = \frac{mass}{molar mass}  

 Molar mass of C₈H₁₈   = 8(12) + 18(1) = 114g/mole

Number of moles of octane  = \frac{11.2}{114}   = 0.098mole

   

    2 mole of octane produced 16 moles of carbon dioxide

    0.098 mole of octane will produce \frac{0.098 x 16}{2}   = 0.79mole of CO₂

Mass of CO₂ = number of moles x molar mass

           Molar mass of CO₂ = 12 + 2(16)  = 44g/mol

Mass of CO₂  = 0.79 x 44  = 34.6g

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