Answer:
The pressure of N₂ gas in cylinder B when compressed at constant temperature increases due to the increase in the frequency of collision between the gas molecules with themselves and with the wall of their container caused by a decrease in volume of the container.
Explanation:
Gas helps to explain the behavior of gases when one or more of either temperature, volume or pressure is varying while the other variables are kept constant.
In the gas cylinder B, the temperature of the given mass of gas is kept constant, however, the volume is decreased by pushing the movable piston farther into the cylinder. According to the gas law by Robert Boyle, the volume of a given mass of gas is inversely proportional to its pressure at constant temperature. This increase in pressure is due to the increase in the frequency of collision between the gas molecules with themselves and with the wall of their container caused by a decrease in volume of the container. As the cylinder becomes smaller, the gas molecules which were spread out further become more packed closely together, therefore, their frequency of collision increases building up pressure in the process.
The chart is attached below and the options are as follow,
A Benzene
B Methanol
C Hexane
D Octane
Answer: Option-B (Methanol) is the correct answer.
Explanation: As we know that the substance given to student is soluble in water. Therefore, those substances which are soluble in water are
polar in nature because water is
polar in nature and
Like Dissolves Like.
Hence, in chart it can easily be seen that
Methanol is also polar in nature due to presence of -O-H (polar) bond. So, the substance will dissolve in it.
Answer:
Final pressure = 0.77atm
Explanation:
The concept used to approach this question is the Ideal gas equation
PV = nRT
where P = pressure
V = Volume
n = number of mole or amount of substance
R = ideal gas constant
T = Temperature in Kelvin
- from the parameters given ; mass = 391g
- Temperature = 695 ∘C = 695 + 273 = 968K
- number of moles = mass/molar mass
- molar mass of CO2 = 12 + 2x16 = 44g/mol
- number of moles = 391g/44g/mol = 8.886mol
plugging into the equation to get the final pressure,
- P = nRT/V = 8.886 x 0.0821 x 968 / 0.770