Te ture hau pai – ngā raruraru me ngā otinga

1. Ahaute mahi tahi i ngā hau i roto i te ipu kati i te tīmatanga he rōrahi V me pāmahana T. The final temperature is 5/4T and the final pēhanga is 2P. What is the final volume of the gas?

Mōhiotia:

Te rōrahi tīmatanga (V₁) = V

Te pāmahana tīmatanga (T₁) = T

Te pāmahana whakamutunga (T₂) = 5/4 T

Pēhanga tuatahi (P₁) = P

Pēhanga whakamutunga (P₂) = 2P

Hiahia: Rōrahi whakamutunga (V₂)

Rongoā:

2. Determine the volume of 2.00 moles of gases (ideal gas) at STP. STP = Standard Temperature and Pressure.

Mōhiotia:

Moles of gas (n) = 2 moles

Te pāmahana paerewa (T) = 0 ^oC = 0 + 273 = 273 Kelvin

Pēhanga paerewa (P) = 1 atm = 1.013 x 10⁵ Pa

Universal gas constant (R) = 8.315 Joule/mole.Kelvin

hiahia : Volume of gases (V)

Rongoā:

Whārite o Ideal gas law (in the number of moles, n)

Volume 2 moles of gases is 44.8 liters.

Volume 1 mol of gases is 45.4 liters / 2 = 22.4 liters.

Volume 1 mol of any gases is 22.4 liters.

3. 4 liters of oxygen gas has a temperature of 27°C and pressure of 2 atm (1 atm = 10⁵ Pa) in a closed container. Universal gas constant (R) = 8.314 J.mole^-1.K^-1 and Avogadro’s number (N_A) = 6.02 x 10²³ molecules/mole. What are the molecules of oxygen gases in the container?

Mōhiotia:

Volume of gases (V) = 4 liters = 4 dm³ = 4x10^-3 m³

Temperature of gases (T) = 27^oC = 27 + 273 = 300 Kelvin

Pressure of gases (P) = 2 atm = 2 x 10⁵ Pa

Universal gas constant (R) = 8.314 J.mole^-1.K^-1

Avogadro’s number (N_A) = 6.02 x 10²³

hiahia : What is the molecules of oxygen gases in the container (N)

Rongoā:

In 1 mole oxygen gases, there are 1.93 x 10²³ oxygen molecules.

4. A container containing a neon gas (Ne, atomic mass = 20 u) at standard temperature and pressure (STP) has a volume of 2 m³. Determine the mass of the neon gas!

Mōhiotia:

Atomic mass of neon = 20 gram/mole = 0,02 kg/mole

Standard temperature (T) = 0^oC = 273 Kelvin

Te pehanga paerewa (P) = 1 atm = 1.013 x 10⁵ Pascal

Volume (V) = 2 m³

hiahia : papatipu (M) of neon gas

Rongoā:

At standard temperature and pressure (STP), 1 mole of any gases, include neon gas, have volume 22.4 ritas = 22.4 dm³ = 0.0448 m³.

In the volume of 2 m³, there are 44.6 moles of neon gas.

Relative atomic mass of neon gas is 20 gram/mole.

This means that in 1 mole there are 20 grams or 0.02 kg of neon gas. Because in 1 mol there are 0.02 kg of neon gas then in 44.6 mole there are 44.6 moles x 0.02 kg/mole = 0.892 kg = 892 gram of neon gases.