Advertisements
Advertisements
Question
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.
Advertisements
Solution
T1 = 6°C + 273 = 279 K
P1 = 4 atm
V1 = 1.5 ml
T2 = 25°C + 273 = 298 K
P2 = 1 atm
V2 = ?
`("P"_1"V"_1)/("T"_1) = ("P"_2"V"_2)/("T"_2)`
V2 = `("P"_1"V"_1)/("T"_1) xx "T"_2/"P"_2`
= `(4 "atm" xx 1.5 "ml" xx 298 "K")/(279 "K" xx 1 "atm")`
V2 = 6.41 ml
APPEARS IN
RELATED QUESTIONS
Convert the following temperature from degree Celcius to kelvin.
−15° C
Convert 101.325 kPa to bar.
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
 |
______________ |
With the help of the graph answer the following -
At constant temperature, Write the statement of law.
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 decreased by 10°C.
Name two items that can serve as a model for Gay Lusaac’s law and explain.
Isochor is the graph plotted between ______.
A gas occupies a volume of 4.2 dm3 at 101 kPa pressure. What volume will gas occupy if the pressure is increased to 235 kPa keeping the temperature constant?
If 2 moles of an ideal gas at 546 K has volume of 44.8 L, then what will be it's pressure? (R = 0.082)
The number of molecules in 8.96 litres of gas at 0°C and 1 atm. pressure is approximately ______.
