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2 years ago

Calculate the number of moles of an ideal gas if it occupies 1750 dm3 under 125,000 Pa at a temperature of 127 C.

Chemistry

2 answers:

andrey2020 [161]2 years ago

6 0

Answer:

65.81

Explanation:

Educere/ Founder's Education Answer

Phoenix [80]2 years ago

5 0

Hey there!

* Converts 1750 dm³ in liters :

1 dm³ = 1 L so 1750 dm³ = 1750 liters

* Convertes 125,000 Pa in atm :

1 Pa = 9.86*10⁻⁶ atm so 9.86*10⁻⁶ / 125,000 => 1.233 atm

* Convertes 127ºC in K :

127 + 273.15 => 400.15 K

R = 0.082 atm.L/mol.K

Finally, it uses an equation of clapeyron :

p * V = n * R * T

1.233 * 1750 = n * 0.082 * 400.15

2157.75 = n * 32.8123

n = 2157.75 / 32.8123

n = 65.76 moles

hope this helps!

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Answer:

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Explanation:

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$Mass=\frac {50}{100}\times 125\ g$

Mass = 62.5 g

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$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus, moles are:

$moles= \frac{62.5\ g}{34\ g/mol}$

$moles= 1.8382\ mol$

Consider the given reaction as:

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Also,

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So,

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The conversion of P(torr) to P(atm) is shown below:
[tex]P(torr)=\frac {1}{760}\times P(atm)$

So,

Pressure = 746 / 760 atm = 0.9816 atm

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The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T₁ = (27 + 273.15) K = 300.15 K

Using ideal gas equation as:

PV=nRT

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9816 atm × V = 0.9191 mol × 0.0821 L.atm/K.mol × 300.15 K

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2 years ago

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