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Alexus [3.1K]
4 years ago
8

A balloon is filled with 5 moles of helium gas. At a pressure of 1.18 atm and a temperature of 303 K, what volume will the gas o

ccupy?
Chemistry
1 answer:
MArishka [77]4 years ago
8 0
Ideal gas law: p·V = n·R·T.<span>
p - pressure of gas; p = 1,18 atm </span>· 101,325 kPa/atm = 119,56 kPa.<span>
V -volume of gas.
n - amount of substance, n(He) = 5 mol.
R - universal gas constant; R = </span>8,314 J/K·mol .<span>
T - temperature of gas; T(He) = 303 K.
From formula of ideal gas law: V = </span>n·R·T / p.
V(He) = 5 mol · 8,314 J/K·mol · 303 K ÷ 119,56 kPa.
V(He) = 105,35 dm³ = 105,35 L.
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A 0.529-g sample of gas occupies 125 ml at 60. cm of hg and 25°c. what is the molar mass of the gas?
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<span>Let's </span>assume that the gas has ideal gas behavior. <span>
Then we can use ideal gas formula,
PV = nRT<span>

</span><span>Where, P is the pressure of the gas (Pa), V is the volume of the gas (m³), n is the number of moles of gas (mol), R is the universal gas constant ( 8.314 J mol</span></span>⁻¹ K⁻¹) and T is temperature in Kelvin.<span>
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</span>P = 60 cm Hg = 79993.4 Pa
V = </span>125  mL = 125 x 10⁻⁶ m³

n = ?

<span> R = 8.314 J mol</span>⁻¹ K⁻¹<span>
T = 25 °C = 298 K
<span>
By substitution,
</span></span>79993.4 Pa<span> x </span>125 x 10⁻⁶ m³ = n x 8.314 J mol⁻¹ K⁻¹ x 298 K<span>
                                          n = 4.0359 x 10</span>⁻³ mol

<span>
Hence, moles of the gas</span> = 4.0359 x 10⁻³ mol<span>

Moles = mass / molar mass

</span>Mass of the gas  = 0.529 g 

<span>Molar mass of the gas</span> = mass / number of moles<span>
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<span>                                    = </span>131.07 g mol</span>⁻¹<span>

Hence, the molar mass of the given gas is </span>131.07 g mol⁻¹

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