The equation of state for a hypothetical ideal gas is known as the ideal gas law, sometimes known as the general gas equation. i.e. PV = nRT or P1V1 = P2V2.
- According to the ideal gas law, the sum of the absolute temperature of the gas and the universal gas constant is equal to the product of the pressure and volume of one gram of an ideal gas.
- Robert Boyle, Gay-Lussac, and Amedeo Avogadro's observational work served as the basis for the ideal gas law. The Ideal gas equation, which simultaneously describes every relationship, is obtained by combining all of their observations into a single statement.
- When applying the gas constant R = 0.082 L.atm/K.mol, pressure, volume, and temperature should all be expressed in units of atmospheres (atm), litres (L), and kelvin (K).
- At high pressure and low temperature, the ideal gas law basically fails because molecule size and intermolecular forces are no longer negligible but rather become significant considerations.
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Answer:
B,D
Explanation:
In December, a city in the Southern Hemisphere has warm weather all month long.
What causes this to happen?
The city experiences fewer hours of daylight.
The city is experiencing a winter solstice.
There is a high concentration of the Sun’s rays in that region.
The Sun reaches its highest point in the sky during this month.In December, a city in the Southern Hemisphere has warm weather all month long.
What causes this to happen?
The city experiences fewer hours of daylight.
The city is experiencing a winter solstice.
There is a high concentration of the Sun’s rays in that region.
The Sun reaches its highest point in the sky during this month.
Solar Radiation(Basically Radiation)
Answer:
Explanation:
These properties are governed by intermolecular forces. The most important part here is the oxygen interaction with the surroundings. For temperature the decreasing order is pentanol, pentanal and pentane. For viscocity: pentanol, pentanal and pentane. For surface tension: pentanol, pentanal and pentane.
This order, as said before, is due to the interaction of oxygen with the surroundings, within the intermolecular forces we can find van der waals forces and hydrogen bonds, it is also know that H-bonds are stronger than van der waals forces so then that is why we have this type of interactions.
