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3 years ago

3) Which pair of formulas represents the empirical formula and molecular

Chemistry

2 answers:

Alexxx [7]3 years ago

6 0

Answer:

The answer to your question is maybe letter D, but the last oxygen needs a number 6.

Explanation:

The empirical formula gives the actual elements that form part of a molecule but not the total numbers.

The molecular formula gives the total number of atoms of each element in a molecule.

We must factor the molecular formula to know if a formula is the empirical formula of that.

A. CH₄ C₂H₆ = 2(CH₃) these are not empirical molecular formulas

B. CH₂O C₄H₆O these are not empirical-molecular formulas

C. O₂ O₃ these are not empirical-molecular formulas

D. C₃H₄O₃ C₆H₈O these are not empirical-molecular formulas

the last oxygen needs a number 6 to be

the answer.

saw5 [17]3 years ago

6 0

D is the correct answer

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Ammonium carbonate decomposes upon heating according to

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The total volume of the gas produced, given the data from the question is 11.84 L

<h3>How to determine the mole of (NH₄)₂CO₃</h3>

Mass of (NH₄)₂CO₃ = 11.83 g
Molar mass of (NH₄)₂CO₃ = 96 g/mol
Mole of (NH₄)₂CO₃ =?

Mole = mass / molar mass

Mole of (NH₄)₂CO₃ = 11.83 / 96

Mole of (NH₄)₂CO₃ = 0.123 mole

<h3>How to determine the volume of NH₃</h3>

Balanced equation

(NH₄)₂CO₃ -> 2NH₃(g) + CO₂(g) + H₂O(g)

From the balanced equation above,

1 mole of (NH₄)₂CO₃ decomposed to produce 2 moles of NH₃

Therefore,

0.123 mole of (NH₄)₂CO₃ will decompose to produce = 0.123 × 2 = 0.246 mole of NH₃

Thus, we can determine the volume of NH₃ produced by using the ideal gas equation as follow:

Temperature (T) = 22 °C = 22 + 273 = 295 K
Pressure (P) = 1.02 bar
Gas constant (R) = 0.08314 bar.L/Kmol
Number of mole (n) = 0.246 moles
Volume of NH₃ (V) =?

PV = nRT

Divide both side by P

V = nRT / P

V = (0.246 × 0.08314 × 295) / 1.02

Volume of NH₃ = 5.92 L

<h3>How to determine the volume of CO₂</h3>

Balanced equation

(NH₄)₂CO₃ -> 2NH₃(g) + CO₂(g) + H₂O(g)

From the balanced equation above,

1 mole of (NH₄)₂CO₃ decomposed to produce 1 moles of CO₂

Therefore,

0.123 mole of (NH₄)₂CO₃ will also decompose to produce = 0.123 mole of CO₂

Thus, we can determine the volume of CO₂ produced by using the ideal gas equation as follow:

Temperature (T) = 22 °C = 22 + 273 = 295 K
Pressure (P) = 1.02 bar
Gas constant (R) = 0.08314 bar.L/Kmol
Number of mole (n) = 0.123 moles
Volume of CO₂ (V) =?

PV = nRT

Divide both side by P

V = nRT / P

V = (0.123 × 0.08314 × 295) / 1.02

Volume of CO₂ = 2.96 L

<h3>How to determine the volume of H₂O</h3>

Balanced equation

(NH₄)₂CO₃ -> 2NH₃(g) + CO₂(g) + H₂O(g)

From the balanced equation above,

1 mole of (NH₄)₂CO₃ decomposed to produce 1 moles of H₂O

Therefore,

0.123 mole of (NH₄)₂CO₃ will also decompose to produce = 0.123 mole of H₂O

Thus, we can determine the volume of H₂O produced by using the ideal gas equation as follow:

Temperature (T) = 22 °C = 22 + 273 = 295 K
Pressure (P) = 1.02 bar
Gas constant (R) = 0.08314 bar.L/Kmol
Number of mole (n) = 0.123 moles
Volume of H₂O (V) =?

PV = nRT

Divide both side by P

V = nRT / P

V = (0.123 × 0.08314 × 295) / 1.02

Volume of H₂O = 2.96 L

<h3>How to determine the total volume of gas produced</h3>

Volume of NH₃ = 5.92 L
Volume of CO₂ = 2.96 L
Volume of H₂O = 2.96 L
Total volume of gas =?

Total volume = 5.92 + 2.96 + 2.96

Total volume of gas = 11.84 L

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