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coldgirl [10]
3 years ago
13

Dumbledore is pleased with your progress. snape is, as always, somewhat indifferent. however, they both feel a gas phase density

problem should come next. calculate the density of helium gas at 25.0◦c and at a pressure of 1521 mmhg. express your answer in g/l.
Chemistry
1 answer:
Zarrin [17]3 years ago
8 0
Answer is: 0,327 g/l.
<span>Ideal gas law: pV = nRT.
</span><span>V - volume, the amount of space occupied by the gas.
</span><span>p - pressure ,1 atm = 760 torr = 760 mmHg.
</span><span>n - amount of substance.
</span>T - temperature, 273 K = 0°<span>C. T = 25 + 273 = 298K.
</span>R - ideal gas constant,<span> R = 0,08206 L</span>·atm/mol·K<span>.
</span>d(He) = M·p ÷ R·T.
d - density.
M - molar mass.
d(He) = 4g/mol · 2atm ÷  298K · 0,08206 L·atm/mol·K = 0,327 g/l.
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Now, with the<u> molar ratio</u> between NaN_3  and N_2  we can <u>calculate the moles</u> of N_2  (2:3), so:

0.054~mol~NaN_3\frac{3~mol~N_2}{2~mol~NaN_3}=0.0819~mol~N_2

With the molar mass of N_2 we can <u>calculate the grams</u>:

0.0819~mol~N_2=\frac{1~mol~N_2}{28~g~N_2}=2.29~g~N_2

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