Answer:
Explanation:
2)
Given data:
Initial volume = 1.50 L
Initial temperature = 20°C
Final temperature = 100°C +20°C = 120°C
Final volume = ?
Solution:
Initial temperature = 20°C = 20+273 = 293 K
Final temperature = 120+273 = 393 K
The given problem will be solve through the Charles Law.
According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.
Mathematical expression:
V₁/T₁ = V₂/T₂
V₁ = Initial volume
T₁ = Initial temperature
V₂ = Final volume
T₂ = Final temperature
Now we will put the values in formula.
V₁/T₁ = V₂/T₂
V₂ = V₁T₂/T₁
V₂ = 1.50 L × 393 K / 293 K
V₂ = 589.5 L.K /293 K
V₂ = 2 L
3)
Given data:
Initial volume = 2.75 dm³
Initial pressure = 455 kpa (455/101 = 4.5 atm)
Initial temperature = 100 °C (100 +273 = 373 K)
Final temperature = 273 K
Final volume = ?
Final pressure = 1 atm
Solution:
Formula:
P₁V₁/T₁ = P₂V₂/T₂
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature
P₂ = Final pressure
V₂ = Final volume
T₂ = Final temperature
Solution:
V₂ = P₁V₁ T₂/ T₁ P₂
V₂ = 4.5 atm × 2.75 dm³ × 273 K / 373 K × 1 atm
V₂ = 3378.375 atm. dm³.K / 373 K.atm
V₂ = 9 dm³
4)
Given data:
Total pressure of mixture = 1023 torr
Pressure of nitrogen = 544 torr
Pressure of oxygen = ?
Solution:
According to the Dalton law of partial pressure,
The pressure of mixture of a gas is the equal to the sum of partial pressure of individual gases.
P(total) = P₁+ P₂ + P₃ +.......+Pₙ
In given question total pressure is 1023 torr and partial pressure of nitrogen is 544 torr.
P(total) = P(N₂)+ P(O₂)
1023 torr = 544 torr + P(O₂)
P(O₂) = 1023 torr - 544 torr
P(O₂) = 479 torr
5)
Given data:
Number of moles of gas = 2.43 mol
Temperature of gas = 35 °C (35+273 = 308 K)
Pressure of gas = 789 torr ( 789/760 = 1.03 atm)
Volume of gas = ?
Solution:
PV = nRT
R = general gas constant = 0.0821 atm.L/ mol.K
V = nRT/P
V = 2.43 mol ×0.0821 atm.L/ mol.K× 308 K / 1.03 atm
V = 61.45 L / 1.03
V = 59.66 L
