Advertisements
Advertisements
Question
Solve the following.
At 25°C and 760 mm of Hg pressure, a gas occupies 600 mL volume. What will be its pressure at the height where the temperature is 10°C and the volume of the gas 640 mL?
Advertisements
Solution
Given:
V1 = Initial volume = 600 mL,
V2 = Final volume = 640 mL
P1 = Initial pressure = 760 mm Hg
T1 = Initial temperature = 25°C = 25 + 273.15 K = 298.15 K
T2 = Final temperature = 10°C = 10 + 273.15 K = 283.15 K
To find: P2 = Final pressure
Formula: `("P"_1"V"_1)/"T"_1=("P"_2"V"_2)/"T"_2`
Calculation:
According to combined gas law,
`("P"_1"V"_1)/"T"_1=("P"_2"V"_2)/"T"_2`
∴ `P_2 = ("P"_1"V"_1"T"_2)/("T"_1"V"_2)`
∴ `P_2 =(760xx600xx283.15)/(298.15xx640)`
∴ P2 = 676.654 mm Hg
The final pressure of a gas is 676.654 mm Hg.
APPEARS IN
RELATED QUESTIONS
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.
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?
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.
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
If the temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes
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 is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)
Give a suitable explanation for the following facts about gases.
Gases don’t settle at the bottom of a container
Would it be easier to drink water with a straw on the top of Mount Everest?
For an ideal gas, at constant temperature and pressure, the volume is ____________.
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?
What is the density of water vapour at boiling point of water?
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?
Which of the following does not represent the ideal gas equation?
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)
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 ______.
Gas equation, pV = nRT is obeyed by a gas in ______.
The SI unit of pressure is ______.
The graph of volume (V) versus absolute temperature (T) at constant pressure is ______.
Gay-Lussac's Law relates pressure and temperature at constant ______.
The ideal gas equation for n moles of gas is ______.
A hot air balloon rises because ______.
According to Boyle's Law, at constant temperature, the pressure of a gas is ______.
An oxygen cylinder of volume 30 litres has 18.20 moles of oxygen. After some oxygen is withdrawn from the cylinder, its gauge pressure drops to 11 atmospheric pressure at temperature 27°C. The mass of the oxygen withdrawn from the cylinder is nearly equal to:
[Given: R = `100/12`Jmol−1 K−1,and molecular mass of 12 O2 = 32, 1 atm pressure = 1.01 × 105 N/m]
