Answer:
n (N₂) = 0.256 mol
n (O₂) = 1.0848 mol
n (Total) = 1.3408 mol
Pressure in new Container = 2.222 atm
Explanation:
Data Given:
For Nitrogen gas (N₂)
Pressure of N₂ gas = 5.23 atm
Volume of N₂ gas = 1.20 L
Temperature of N₂ gas = 26° C
Temperature of N₂ gas in Kelven (K) = 26° C +273
Temperature of N₂ gas in Kelven (K) = 299K
ideal gas Constant R = 0.08206 L atm K⁻¹ mol⁻¹
quantity of gas N₂ gas = ?
For Oxygen gas (O₂)
Pressure of O₂ gas = 5.21 atm
Volume of O₂ gas = 5.21 L
Temperature of O₂ gas = 26° C
Temperature of O₂ gas in Kelven (K) = 26° C +273
Temperature of O₂ gas in Kelven (K) = 299K
ideal gas Constant R = 0.08206 L atm K⁻¹ mol⁻¹
quantity of gas O₂ gas = ?
*we also have to find the total Pressure in the new container = ?
Formula Used
PV =nRT
n (N₂) = PV /RT . . . . . . . . . . . . . (1)
* Find the quantity of N₂
Put value in formula (1)
n (N₂) = 5.23 atm x 1.20 L / 0.08206 L atm K⁻¹ mol⁻¹ x 299K
n (N₂) = 6.276 atm .L / 24.52 L atm. mol⁻¹ x 299K
n (N₂) = 0.256 mol
* Find the quantity of O₂
Put value in formula (1)
n (O₂) = 5.21 atm x 5.10 L / 0.08206 L atm K⁻¹ mol⁻¹ x 299K
n (O₂) = 26.6 atm .L / 24.52 L atm. mol⁻¹
n (O₂) = 1.0848 mol
*Now to find the Total Quantity of both gases
n(Total) = n (N₂) + n (O₂)
n (Total) = 0.256 mol + 1.0848 mol
n (Total) = 1.3408 mol
**To find the Total Pressure in the new Container
Data to calculate Total Pressure in new container
Volume of gas = 14.5 L
Temperature of gases = 20° C
Temperature of gases in Kelven (K) = 20° C +273
Temperature of gases in Kelven (K) = 293K
ideal gas Constant R = 0.08206 L atm K⁻¹ mol⁻¹
Volume Pressure in new container = ?
Formula Used
PV =nRT
P = nRT / V . . . . . . . . . . . . . (2)
Put values in Equation (2)
P = 1.3408 mol x 0.08206 L atm K⁻¹ mol⁻¹ x 293 K / 14.5 L
P = 2.222 atm
