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There are three main gas laws: Boyle's, Charles' and the pressure law. These describe the relationship between pressure, volume and temperature of an ideal gas.
Boyle's law: the volume of a gas is inversely proportional to its pressure; i.e. doulbing the pressure applied to a gas will halve the volume it takes up (and vice-versa).
Charles' law: the volume of a gas is directly proportional to its temperature; i.e. doulbing the temperature of a gas will double the volume it takes up (and vice-versa).
Pressure law: the pressure of a gas is directly proportional to its temperature; i.e. doubling the temperature of a gas will double the pressure placed upon the gas (and vice-versa).
These three laws can be combined with another to give the ideal gas law: PV = nRT (where P = pressure, V = volume, n = number of moles, R = universal gas constant and T = temperature in Kelvin).
But seriously, next time, just Google it - it'll be faster. Or maybe read a textbook?
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What are the 2 factors that affect gas preassure?
There are four factors that affect gas pressure. The ideal gas law enumerates them: Pressure = number of gas molecules * constant describing the particular gas's behavior * temperature of the gas / volume in which the gas is confined
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
Gases show least ideal behaviour at 1- high pressure and 2- low temperature.
When is H2 an ideal gas?
low pressure and high temperature
How does decreasing the gas volume affect the pressue of a gas?
Assuming temperature and moles of gas remains the same, then decreasing the volume of the gas will increase the pressure. Decreasing the volume enough will result in non ideal behavior.
How does ammonia gas liquefied?
You have to give ideal pressure and temperature. It liquefied in that conditions.
What are the 2 factors that affect gas preassure?
There are four factors that affect gas pressure. The ideal gas law enumerates them: Pressure = number of gas molecules * constant describing the particular gas's behavior * temperature of the gas / volume in which the gas is confined
What is an imaginary gas that conforms perfectly to the kinetic molecular theory callled?
That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
Gases show least ideal behaviour at 1- high pressure and 2- low temperature.
When is H2 an ideal gas?
low pressure and high temperature
Is pressure independent of temperature?
The relationship between pressure and temperature depends on the conditions and the substance involved. In general, for ideal gases, pressure and temperature are related by the ideal gas law, which is given by the equation: � � = � � � , PV=nRT, where: � P is the pressure, � V is the volume, � n is the number of moles of gas, � R is the ideal gas constant, and � T is the temperature in kelvin. According to the ideal gas law, pressure is directly proportional to temperature when other parameters are held constant. This means that, for an ideal gas, if the temperature increases while other factors remain constant, the pressure will also increase, and vice versa. However, for real gases and under certain conditions, the relationship between pressure and temperature can be more complex, and deviations from ideal behavior may occur. In some cases, other factors such as intermolecular forces and the nature of the substance can affect the relationship between pressure and temperature. Therefore, it's important to consider the specific conditions and properties of the substance in question.
What gas conforms to the gas laws at all conditions of temperature and pressure?
The ideal gas law
What happens to the gas when temperature drops from 100 degrees to -100 degrees?
You will recall from the Ideal Gas Laws that temperature, pressure, and volume are all connected in terms of the behavior of a gas (especially an ideal gas, but actual gas resembles ideal gas to a certain extent). So, if the gas is in a container of fixed volume, then reducing the temperature will correspondingly reduce the pressure.
What happens to gas pressure when temperature rises?
If the volume remains constant, the pressure will increase as the temperature increases. In an ideal gas (under normal conditions, gases have a behavior that's close to that of an ideal gas), the pressure is directly proportional to the temperature. Assuming, of course, that the temperature is measured in Kelvin.
The volume of a gas is directly proportional to the number of moles of that gas if?
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
What are factors that affect gas pressure?
There are two factors that affect gas pressure. These factors are temperature and volume. Higher volume means lower pressure. Higher temperature means higher pressure.
What does the ideal gas law not specify?
What does the ideal gas law not specify the density and mass of the gas. It instead deals with volume, temperature and pressure.
What is the temperature at which an ideal gas occupies zero pressure?
Absolute Zero
