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2 years ago

5

A compound is known to contain only carbon, hydrogen, and oxygen. If the complete combustion of a 0.150-g sample of this compoun

d produces 0.225 g of CO2 and 0.0614 g of H2O, what is the empirical formula of this compound

2 answers:

Rzqust [24]2 years ago

8 0

Answer: the empirical formula is C3H4O3

Explanation:Please see attachment for explanation

egoroff_w [7]2 years ago

3 0

Answer:

The answer to your question is C₃H₄O₃

Explanation:

Data

CxHyOz

mass of sample = 0.150 g

mass of CO₂ = 0.225 g

mass of H₂O = 0.0614 g

Reaction

CxHyOz + O₂ ⇒ CO₂ + H₂O

Process

1.- Calculate the moles of C

44 g of CO₂ ----------------- 12 g of C

0.225 g ---------------- x

x = (0.225 x 12) / 44

x = 0.0614 g of C

12 g of C -------------------- 1 mol

0.0614 g of C --------------- x

x = 0.0051 moles of Carbon

2.- Calculate the moles of hydrogen

18 g of H₂O ------------------ 2 g of H

0.0614 g --------------- x

x = 0.0068 g of H

1 g of H ----------------------- 1 mol of H

0.0068 g --------------------- x

x = 0.0068 moles of H

3.- Calculate the mass of Oxygen

Mass of oxygen = 0.150 - 0.0614 - 0.0068

= 0.0818 g

16 g of O ------------------- 1 mol

0.0818 g -------------------- x

x = (0.0818 x 1) / 16

x = 0.0051 moles of O

4.- Divide by the lowest number of moles

Carbon 0.0051 / 0.0051 = 1

Hydrogen 0.0068 / 0.0051 = 1.33

Oxygen 0.0051 / 0.0051 = 1

Multiply these numbers by 3

Carbon 3

Hydrogen = 4

Oxygen = 3

5.- Write the empirical formula

C₃H₄O₃

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Answer:

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Explanation:

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46.2kg × 1,000g/kg = 46,200g

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number of moles = mass in grams / molar mass

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a) Balanced chemical equation (given):

C₈H₁₈ (l) + ²⁵/₂ O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)

b) mole ratio:

1 mol C₈H₁₈ / 8 mol CO₂ = 404.55 mol C₈H₁₈ / x

Solve for x:

x = 404.55mol C₈H₁₈ × 8 mol CO₂ / 1mol C₈H₁₈ = 3,236.4 mol CO₂

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Use the ideal gas equation:

pV = nRT

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Now put all the given values in the above formula, we get:

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The formula used for $\Delta G_{rxn}$ is:

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$A(aq)\rightleftharpoons B(aq)$

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