Advertisements
Advertisements
Question
Solve the following.
Nitrogen gas is filled in a container of volume 2.32 L at 32°C and 4.7 atm pressure. Calculate the number of moles of the gas.
Advertisements
Solution
Given:
V = 2.32 L,
P = 4.7 atm,
T = 32°C = 32 + 273.15 K = 305.15 K
R = 0.0821 L atm K−1 mol−1
To find: n = number of moles of gas
Formula: PV = nRT
Calculation:
According to the ideal gas equation,
PV = nRT
∴ n = `"PV"/"RT"`
∴ n = `(4.7xx2.32)/(0.0821xx305.15)`
∴ n = 0.435 moles
Number of moles of N2 gas in the given volume is 0.435 moles.
APPEARS IN
RELATED QUESTIONS
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 pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is
The value of the gas constant R is
Consider the following statements
i) Atmospheric pressure is less at the top of a mountain than at sea level
ii) Gases are much more compressible than solids or liquids
iii) When the atmospheric pressure increases the height of the mercury column rises
Select the correct statement
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?
Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.
The variation of volume V, with temperature T, keeping the pressure constant is called the coefficient of thermal expansion ie α = `1/"V"((∂"V")/(∂"T"))_"P"`. For an ideal gas α is equal to
What are ideal gases?
Give a suitable explanation for the following facts about gases.
Gases don’t settle at the bottom of a container
Why do astronauts have to wear protective suits when they are on the surface of the moon?
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.
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 ____________.
At constant pressure, a quantity of an ideal gas occupies 1.0 × 10−2 dm3 volume at 200 K. At what temperature, the volume will be 2.0 × 10−3 dm3?
At a constant pressure, the density of a certain amount of an ideal gas is ____________.
If 10−4 dm3 of water is introduced into a 1 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?
(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 JK−1 mol−1)
In Duma's method, 0.52 g of an organic compound on combustion gave 68.6 mL N2 at 27°C and 756 mm pressure. What is the percentage of nitrogen in the compound?
Gas equation, pV = nRT is obeyed by a gas in ______.
The ideal gas equation for n moles of gas is ______.
The value of the universal gas constant R is ______.
A pressure cooker works on the principle of ______.
According to Boyle's Law, at constant temperature, the pressure of a gas is ______.
