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Sauron [17]
3 years ago
11

Mass

Chemistry
1 answer:
DiKsa [7]3 years ago
7 0

The molecular formula =C₆H₁₂O₆

<h3>Further explanation</h3>

Given

6.00 g of a certain compound X

The molecular molar mass of 180. g/mol

CO₂=8.8 g

H₂O=3.6 g

Required

The molecular formula

Solution

mass C in CO₂ :

= 1.12/44 x 8.8

= 2.4 g

mass H in H₂O :

= 2.1/18 x 3.6

= 0.4 g

Mass O in compound :

= 6-(2.4+0.4)

= 3.2 g

Mol ratio C : H : O

= 2.4/12 : 0.4/1 : 3.2/16

= 0.2 : 0.4 : 0.2

= 1 : 2 : 1

The empirical formula : CH₂O

(CH₂O)n=180 g/mol

(12+2+16)n=180

(30)n=180

n=6

(CH₂O)₆=C₆H₁₂O₆

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choli [55]

Answer:

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Explanation:

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The equation for the reaction is expressed as:

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The ICE Table is shown below as follows:

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Change (M)         - 0.04          -0.04                          + 0.04

Equilibrium (M)      0.04             0                                0.04

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K_a = \frac{10^{-14}}{K_b}

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<h3>Stoichiometric problem</h3>

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More on stoichiometric problems can be found here: brainly.com/question/14465605

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