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3 years ago

What is the density of chlorine gas (MM = 71.0glmol) at 1.50 atm and 25.0C

Chemistry

1 answer:

IrinaVladis [17]3 years ago

5 0

Answer: D=4.35g/L

Explanation:

The formula for density is $D=\frac{M}{V}$ . M is mass in grams and V is volume in liters.

Since we are give pressure and temperature, we can use the ideal gas law to find moles/volume. FInding moles/volume would give us the base for density. All we would have to do is convert moles to grams.

Ideal Gas Law: PV=nRT

$\frac{n}{V} =\frac{P}{RT}$

$\frac{n}{V}=\frac{1.50 atm}{(0.08206Latm/Kmol)(25+274.15K)}$

$\frac{n}{V} =\frac{0.061309mol}{L}$

Now that we have moles, we can use molar mass of chlorine gas to find grams.

$0.061309mol*\frac{71.0g}{mol} =4.3529g$

With our grams, we can find our density.

$D=\frac{4.3529g}{L}$

We need correct significant figures so our density is:

$D=\frac{4.35g}{L}$

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The question is incomplete, here is the complete question:

Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume of hydrogen chloride would be produced by this reaction if 1.1 mL of methane were consumed? Be sure your answer has the correct number of significant digits.

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Explanation:

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