V1/T1=V2/T2
524 cm^3/491 K =V2/297K
V2=(524 cm^3*297K)/491 K= 317K
1.0 mole of gas at STP occupies 22.4 Litres.
4/0L / 22.4 L/mole = 0.179 moles He.
Answer:
409 g/mol
Explanation:
you divide the mass by the moles to get the molar mass
Answer:
V₂ = 648.53 mL
Explanation:
Given data:
Initial volume of gas = 490. mL
Initial temperature = -35°C (-35 + 273 = 238 k)
Final temperature = 42°C = (42+273 = 315 k)
Final volume = ?
Solution:
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 = 490 mL × 315 K / 238 k
V₂ = 154350 mL.K / 238 K
V₂ = 648.53 mL
