Advertisements
Advertisements
प्रश्न
Solve the following.
A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5g neon. If the pressure of the mixture of the gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture?
उत्तर
Given:
mO2 = 70.6 g,
mNe = 167.5 g,
PTotal = 25 bar
To find: Partial pressure of each gas
Formula: P1 = x1 × PTotal
Calculation:
Determine number of moles (n) of each gas using formula:
n = `"m"/"M"`
∴ nO2 = `(70.6 "g")/(32 "g mol"^-1)` = 2.206 mol
nNe = `(167.5 "g")/(20 "g mol"^-1)` = 8.375 mol
Determine the mole fraction of each gas using the formula:
x = `"n"/("n"_"Total")`
`""^"x""O"_2=(""^"n""O"_2)/(""^"n""O"_2+"n"_"Ne")=(2.206 "mol")/((2.206+8.375) "mol")=(2.206 "mol")/(10.581 "mol")=0.208`
xNe = `("n"_"Ne")/("n"_"Total")=(8.375 "mol")/(10.581 "mol")` = 0.792
Calculate the partial pressure of each gas:
PO2 = xO2 × PTotal = 0.208 × 25 bar = 5.2 bar
PNe = xNe × PTotal = 0.792 × 25 bar = 19.8 bar
The partial pressure of dioxygen and neon are 5.2 bar and 19.8 bar respectively.
APPEARS IN
संबंधित प्रश्न
Answer in one sentence.
The pressure that each individual gas would exert if it were alone in the container, what do we call it as?
Answer in one sentence.
When a gas is heated the particles move more quickly. What is the change in the volume of a heated gas if the pressure is kept constant?
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 volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
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.
Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is
A bottle of ammonia and a bottle of HCl connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be
If the temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes
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?
What is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)
What are ideal gases?
Suggest why there is no hydrogen (H2) in our atmosphere. Why does the moon have no atmosphere?
Would it be easier to drink water with a straw on the top of Mount Everest?
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 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.
At constant temperature, a quantity of an ideal gas occupies 50 mL at 500 mmHg pressure. At what pressure, the volume will be 100 mL?
At a constant pressure, an ideal gas has a volume of 200 cm3 at 25°C. If the gas is cooled to −3°C, what will be the final volume of a gas?
The density of an ideal gas can be expressed as d = ____________.
At a constant pressure, the density of a certain amount of an ideal gas 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)
A box contains 0.90 g of liquid water in equilibrium with water vapour at 27°C. The equilibrium vapour pressure of water at 27°C is 32.0 Torr. When the volume of the box is increased, some of the liquid water evaporates to maintain the equilibrium pressure. If the liquid water evaporates, then the volume of the box must be - litre (nearest integer) R = 0.0821 L atm K-1 mol-1.
(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas)
Which of the following graphs is not correct for ideal gas?
An evacuated glass vessel weighs 40 g when empty, 135 g when filled with a liquid of density 0.95 g mL−1 and 40.5 g when filled with an ideal gas at 0.82 atm at 250 K. The molar mass of the gas in g mol−1 is ______.
(Given: R = 0.082 L atm K−1 mol−1)
120 g of an ideal gas of molecular weight 40 g mol−1 are confined to a volume of 20 L at 400 K.
Using R = 0.0821 L atm K−1 mol−1, the pressure of the gas is ______.
A gas is heated from 273 K to 373 K at 1 atm pressure. If the initial volume of the gas is 10 L, its final volume would be ______.
