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3 years ago

What volume of carbon dioxide gas can be collected from

Chemistry

1 answer:

alisha [4.7K]3 years ago

7 0

Answer:

1.22 L of carbon dioxide gas

Explanation:

The reaction that takes place is:

CaCO₃ + HCl → CaCl₂ + CO₂ + H₂O

First we <u>determine which reactant is limiting</u>:

Calcium carbonate ⇒ 10.0 g CaCO₃ ÷ 100 g/mol = 0.10 mol CaCO₃

Hydrochloric acid ⇒ 0.100 L * 0.50 M = 0.05 mol HCl

So HCl is the limiting reactant.

Now we calculate the moles of CO₂ produced:

0.05 mol HCl * $\frac{1molCO_{2}}{1molHCl}$ = 0.05 mol CO₂

Finally we use PV=nRT to <u>calculate the volume</u>:

P = 1 atm

n = 0.05 mol

T = 25 °C ⇒ 25 + 273.16 = 298.16 K

1 atm * V = 0.05 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K

V = 1.22 L

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Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°

Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).

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n = m/M (m is the mass, and M the molar mass)

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$PxM = \frac{m}{V}RT$

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$Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}$

And,

$y_{NO2} + y_{N2O4} = 1$

$y_{N2O4} = 1 - y_{NO2}$

So,

$68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})$

$68.0687 - 92 = 46y_{NO2} - 92y_{NO2}$

$46y_{NO2} = 23.9313$

$y_{NO2} = 0.52$

$y_{N2O4} = 0.48$

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

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