Advertisements
Advertisements
प्रश्न
Solve the following.
The volume of a given mass of a gas at 0°C is 2 dm3. Calculate the new volume of the gas at constant pressure when the temperature is increased by 10°C.
Advertisements
उत्तर
Given:
T1 = Initial temperature = 0°C = 0 + 273.15 = 273.15 K,
V1 = Initial volume = 2 dm3
T2 = Final temperature = 273.15 K + 10 = 283.15 K
To find: V2 = Final volume
Formula: `"V"_1/"T"_1="V"_2/"T"_2` (at constant n and P)
Calculation:
According to Charles’ law,
`"V"_1/"T"_1="V"_2/"T"_2` (at constant n and P)
∴ V2 = `("V"_1"T"_2)/"T"_1=(2xx283.15)/273.15` = 2.073 dm3
The new volume of a given mass of gas is 2.073 dm3
APPEARS IN
संबंधित प्रश्न
State (i) the three variables for gas laws and (ii) SI units of these variables.
Give reason for the following:
Gases have a lower density compared to solids or liquids.
Answer in one sentence.
A bubble of methane gas rises from the bottom of the North sea. What will happen to the size of the bubble as it rises to the surface?
Convert the following pressure value into Pascals.
107000 Nm−2
Convert the following pressure value into Pascals.
1 atmosphere
Convert −100° C to kelvin
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
 |
______________ |
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
 |
______________ |
Consider a sample of a gas in a cylinder with a movable piston.
Show diagrammatically the changes in the position of the piston, if the temperature is decreased from 300 K to 150 K at constant pressure.
With the help of the graph answer the following -
At constant temperature, Write the statement of law.
Solve the following.
A balloon is inflated with helium gas at room temperature of 25°C and at 1 bar pressure when its initial volume is 2.27L and allowed to rise in the air. As it rises in the air external pressure decreases and the volume of the gas increases till finally, it bursts when external pressure is 0.3bar. What is the limit at which the volume of the balloon can stay inflated?
The temperatures at which real gases obey the ideal gas laws over a wide range of pressure is called __________.
Use of hot air balloon in sports and meteorological observation is an application of
Explain the following observation.
The type of an automobile is inflated to slightly lesser pressure in summer than in winter
A sample of gas has a volume of 8.5 dm3 at an unknown temperature. When the sample is submerged in ice water at 0°C, its volume gets reduced to 6.37 dm3. What is its initial temperature?
Of two samples of nitrogen gas, sample A contains 1.5 moles of nitrogen in a vessel of the volume of 37.6 dm3 at 298 K, and sample B is in a vessel of volume 16.5 dm3 at 298 K. Calculate the number of moles in sample B.
Sulphur hexafluoride is a colourless, odourless gas; calculate the pressure exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 dm3 at 69.5 °C, assuming ideal gas behaviour
A small bubble rises from the bottom of a lake where the temperature and pressure are 6°C and 4 atm. to the water surface, where the temperature is 25°C and pressure is 1 atm. Calculate the final volume in (mL) of the bubble, if its initial volume is 1.5 mL.
Hydrochloric acid is treated with a metal to produce hydrogen gas. Suppose a student carries out this reaction and collects a volume of 154.4 × 10−3 dm3 of a gas at a pressure of 742 mm of Hg at a temperature of 298 K. What mass of hydrogen gas (in mg) did the student collect?
At 25°C and 1 atm, a cylinder containing 10 L of an ideal gas is connected to the empty cylinder with a capacity of 20 L. The pressures exerted by gas m both the cylinders will be ____________.
A certain sample of gas has a volume of 0.2 L at one atmosphere pressure and 273.15 K. What is the volume of gas at 273.15°C at same pressure?
According to Andrews isothermals at what temperature the carbon dioxide gas starts to condense at 73 atmosphere?
Isochor is the graph plotted between ______.
If 300 mL of a gas at 26.85°C is cooled to 6.85°C at constant pressure. What will be the final volume of gas?
