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3 years ago

How many moles of helium gas are contained in a 4.0-L flask at STP?

Chemistry

2 answers:

ExtremeBDS [4]3 years ago

7 0

Answer:

0.1784 moles of helium gas are contained in a 4.0-L flask at STP.

Explanation:

At STP. temperature of the helium gas = T = 273.15 K

At STP, pressure of the helium gas = P = 1 atm

Volume of the helium gas at STP = V = 4.0 L

Moles of the helium gas = n

Using an ideal gas equation :

$PV=nRT$

$n=\frac{PV}{RT}=\frac{1 atm\times 4.0 L}{0.0821 atm L/mol K\times 273.15 K}$

n = 0.1784 mol

0.1784 moles of helium gas are contained in a 4.0-L flask at STP.

mel-nik [20]3 years ago

4 0

1.0 mole of gas at STP occupies 22.4 Litres.
4/0L / 22.4 L/mole = 0.179 moles He.

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Explain why a fluorescent light bulb is not as hot as an incandescent light bulb.

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Therefore, a fluorescent light bulb is not as hot as an incandescent light bulb.

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3 years ago

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2) Convert 2.65*10^ ^ 25 atoms of Chlorine to moles of CI

Irina18 [472]

Answer:

22 mol

Explanation:

Given data:

Number of atoms of Cl = 2.65×10²⁵ atom

Number of moles of Cl = ?

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance. The number 6.022 × 10²³ is called Avogadro number.

1 mole = 6.022 × 10²³ atoms

2.65×10²⁵ atom × 1 mol / 6.022 × 10²³ atoms

0.44×10² mol

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3 years ago

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Option C, Antarctic Treaty System, is the right answer.

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3 years ago

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If the initial temperature of a movable cylinder was 50 degrees Celsius

slega [8]

Answer:

8.45 L

Explanation:

From the question given above, the following data were obtained:

Initial temperature (T₁) = 50 °C

Initial pressure (P₁) = 2 atm

Initial volume (V₁) = 5 L

Final temperature (T₂) = 0 °C

Final pressure (P₂) = 1 atm

Final volume (V₂) =?

Next, we shall convert celsius temperature to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T₁) = 50 °C

Initial temperature (T₁) = 50 °C + 273

Initial temperature (T₁) = 323 K

Final temperature (T₂) = 0 °C

Final temperature (T₂) = 0 °C + 273

Final temperature (T₂) = 273 K

Finally, we shall determine the new volume. This can be obtained as follow:

Initial temperature (T₁) = 323 K

Initial pressure (P₁) = 2 atm

Initial volume (V₁) = 5 L

Final temperature (T₂) = 273 k

Final pressure (P₂) = 1 atm

Final volume (V₂) =?

P₁V₁ / T₁ = P₂V₂ / T₂

2 × 5 / 323 = 1 × V₂ / 273

10 / 323 = V₂ / 273

Cross multiply

323 × V₂ = 10 × 273

323 × V₂ = 2730

Divide both side by 323

V₂ = 2730 / 323

V₂ = 8.45 L

Thus, the new volume is 8.45 L

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3 years ago

A certain water tower hold 4.6×10^5 gallons of water. find the volume of that water in liters.

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Explanation:

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