Advertisements
Advertisements
Question
A tank contains a mixture of 52.5 g of oxygen and 65.1 g of CO2 at 300 K the total pressure in the tanks is 9.21 atm. Calculate the partial pressure (in atm.) of each gas in the mixture.
Advertisements
Solution
`"m"_("O"_2)` = 52.5 g
`"P"_("O"_2)` = ?
`"m"_("CO"_2)` = 65.1 g
`"P"_("CO"_2)` = ?
T = 300 K
P = 9.21 atm
`"P"_("O"_2) = "X"_("O"_2) xx "Total Pressure"`
`"X"_("O"_2) = "n"_("O"_2)/("n"_("O"_2) + "n"_("CO"_2))`
`"n"_("O"_2) = "Mass of O"_2/("Molar mass of O"_2)`
= `(52.5 "g")/(32 "g mol"^-1)`
= 1.64 mol
`"n"_("CO"_2) = "Mass of CO"_2/"Molar mass of CO"_2`
= `(65.1 "g")/(44 "g mol"^-1)`
= 1.48 mol
`"X"_("O"_2) = "n"_("O"_2)/("n"_("O"_2) + "n"_("CO"_2))`
= `1.64/3.12`
= 0.53
`"X"_("CO"_2) = "n"_("CO"_2)/("n"_("O"_2) + "n"_("CO"_2))`
= `1.48/3.12`
= 0.47
`"P"_("O"_2) = "X"_("O"_2) xx "Total Pressure"`
= 0.53 × 9.21 atm
= 4.88 atm
`"P"_("CO"_2) = "X"_("CO"_2) xx "Total Pressure"`
= 0.47 × 9.21 atm
= 4.33 atm
APPEARS IN
RELATED QUESTIONS
If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?
Solve the following.
Calculate the number of molecules of methane in 0.50 m3 of the gas at a pressure of 2.0 × 102 kPa and a temperature of exactly 300 K.
At identical temperature and pressure, the rate of diffusion of hydrogen gas is `3sqrt3` times that of a hydrocarbon having molecular formula CnH2n–2. What is the value of n?
Argon is an inert gas used in light bulbs to retard the vaporization of the tungsten filament. A certain light bulb containing argon at 1.2 atm and 18°C is heated to 85°C at constant volume. Calculate its final pressure in atm.
A combustible gas is stored in a metal tank at a pressure of 2.98 atm at 25°C. The tank can withstand a maximum pressure of 12 atm after which it will explode. The building in which the tank has been stored catches fire. Now predict whether the tank will blow up first or start melting? (Melting point of the metal = 1100 K).
A cold drink bottle contains 200 mL liquid, in which CO2 is 0.1 molar. Considering CO2 as an ideal gas the volume of the dissolved CO2 at S.T.P is ______.
For an ideal gas, at constant temperature and pressure, the volume is ____________.
If two moles of an ideal gas at 546 K occupy a volume of 44.8 L. What is the pressure of ideal gas at 546 K? (R = 0.0821 L atm mol-1 K-1)
Which of the following does not represent the ideal gas equation?
The graph of volume (V) versus absolute temperature (T) at constant pressure is ______.
