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White raven [17]
3 years ago
7

For neon, determine the moles and mass contained in a 29.9−L volume at a pressure of 481.1 torr at a temperature of 300.0 K.

Chemistry
1 answer:
kondor19780726 [428]3 years ago
8 0

Answer:

.7689 mol

15.516 g

Explanation:

Use the Ideal Gas Law, PV = nRT.

Make sure to use the correct ideal gas constant R. You can either put R in torr, or you can change the pressure to atm. I've just used the torr ideal gas constant.

481.1 torr * 29.9 L = n 62.364 LTorr/molK * 300 K

14384.89 = 18709.2n

n = <u>.7689 mol</u>

The molar mass of neon (remember that neon gas = Ne, it's not diatomic) is 20.18 g/mol from the periodic table.

.7689 mol * 20.18 g/mol = <u>15.516 g</u>

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Explanation:

Using Ideal gas equation for same mole of gas as

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Given ,  

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P₁ = 2575 mm Hg

Also, P (atm) = P (mm Hg) / 760

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Using above equation as:

\frac {{P_1}\times {V_1}}{T_1}=\frac {{P_2}\times {V_2}}{T_2}

\frac{{3.39}\times {25.0}}{353}=\frac{{1.35}\times {V_2}}{253}

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Solving for V₂ , we get:

<u>V₂ = 45.0 L</u>

45.0 L is the volume of gas will the balloon contain at 1.35 atm and 253 K.

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Explanation:

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The equation is,

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P_2 = final pressure of gas = ?

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