Advertisements
Advertisements
प्रश्न
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).
Advertisements
उत्तर
Pressure of the gas in the tank at its melting point
T = 298 K; P1 = 2.98 atom; T2 = 1100 K; P2 = ?
`"P"_1/"T"_1 = "P"_2/"T"_2`
P2 = `"P"_1/"T"_1 xx "T"_2`
= `(2.98 "atm")/(298 "K") xx 1100 "K"`
= 11 atm
At 1100 K the pressure of the gas inside the tank will become 11 atm. Given that tank can withstand a maximum pressure of 12 atm, the tank will start melting first.
APPEARS IN
संबंधित प्रश्न
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.
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.
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?
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.
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?
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)
A hot air balloon rises because ______.
