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What else can I help you with?
When does raising the temperature of a gas increase its preasure?
This is the Gay-Lussac law: at constant volume of a gas the temperature increase when the pressure increase.
What happens to the temperature if you add a mole of gas?
If you add a mole of gas to a closed system at constant volume, the temperature will increase if the pressure remains constant due to the increase in internal energy of the system. If the volume is allowed to expand and the pressure is constant, the temperature may stay the same or decrease, depending on the conditions of the system.
Why would the pressure of a sample of gas at a constant volume fall mm Hg?
The pressure of a gas at constant volume can fall due to a decrease in temperature, as described by Gay-Lussac's law. When the temperature of the gas decreases, the kinetic energy of the gas molecules reduces, leading to fewer collisions with the container walls and consequently lower pressure. Additionally, if the gas is allowed to expand or if there are any leaks in the system, the pressure would also decrease.
What happens to volume when pressure is doubled?
The pressure of a gas would be reduced by half if the volume of the container doubled, provided that no other change occurred. Pressure and volume are inversely proportional. The relationship between the two is known as Boyle's law. In brief, the volume of a gas changes inversely with the pressure of the gas if the temperature and quantity of gas remain constant.
If pressure is applied to a confined volume of gas the temperature of that gas will increase. Will that in effect negate Boyle's law?
By "confined" it is assumed that no heat exchange is allowed. This is sometimes called an "adiabatic" change. P V = R T still applies, but since the temperature changes, P x V is no longer constant. The relation for adiabatic changes is often expressed as P x V^gamma = constant, where gamma is is a constant and the ^ sign means "raised to the power". Using algebra these 2 equations can be combined to eliminate one of the variables P or V, to give relationships between V and T, or between P and T. "Negate" is too strong a word here. Boyle's law refers to constant temperature, so it cannot be used when the temperature changes. When you compress a gas at constant temperature, heat passes out. If it is thermally isolated the heat is retained and shows up as a rise in temperature.
How is isothermal possible in a balloon?
Isothermal is where pressure and/or volume changes, but temperature remains constant. Pressure, Volume, and Temperature are related as: PV = nRT =NkT for an ideal gas. Here, we see that since a balloon's volume is allowed to change, its pressure remains relatively constant. Whenever there is a pressure change, it'll be offset by an equivalent change in volume, thus temperature is constant.
When does raising the temperature of a gas increase its preasure?
This is the Gay-Lussac law: at constant volume of a gas the temperature increase when the pressure increase.
What happens to the temperature if you add a mole of gas?
If you add a mole of gas to a closed system at constant volume, the temperature will increase if the pressure remains constant due to the increase in internal energy of the system. If the volume is allowed to expand and the pressure is constant, the temperature may stay the same or decrease, depending on the conditions of the system.
What would be the pressure in mm Hg if this gas was allowed to expand to 975 ml at a constant temperature?
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'
What is a factor held constant?
In science, as in real life sometimes several 'factors' effect the outcome of an experiment. In order to make the problem easier to study one or more of these is 'held constant' or not allowed to change in order to see the effect of the other variables. EX. Gas volume can be effected by both pressure and temperature. In order to understand the effect of pressure, Boyle kept the temperature constant. He then changed the pressure to see what happened to the volume of a gas. This gave him what is now called Boyle's Law: The volume of a gas varies inversely as the pressure when the temperature is held constant.
What factor is held constant?
In science, as in real life sometimes several 'factors' effect the outcome of an experiment. In order to make the problem easier to study one or more of these is 'held constant' or not allowed to change in order to see the effect of the other variables. EX. Gas volume can be effected by both pressure and temperature. In order to understand the effect of pressure, Boyle kept the temperature constant. He then changed the pressure to see what happened to the volume of a gas. This gave him what is now called Boyle's Law: The volume of a gas varies inversely as the pressure when the temperature is held constant.
What change in volume would cause the pressure of an enclosed gas to be reduced toone quarter of its original value?
This is the reduction of volume to one-third.
When the temperature is constant gas volume will decrease as the pressure decreases is that true?
If I remember correctly it is a little more complicated than that. The general equation PV=nRT for an ideal gas is elementary knowledge. The fact is that when you increase temperature many things can happen. It depends on how you treat your system. In general if you increase temperature in an open system the pressure will remain fairly constant, but the volume will increase. If it is a closed system in which the volume is not allowed to expand the pressure will increase with increased temperature. You also have to remember chemical properties also such as phase changes. Hope that rambling mess helps lol.
What happend to air when it is compressed or allowed to expand?
When air is allowed to expand, it cools, and when it is compressed, it warms. Additional Information: Contraction, like compression is shrinkage that can actually be caused by cooling and should not be confused with compression.
A gas with a volume of 4.00 L at a pressure of 205 kPa is allowed to expand to a volume of 12.0 L. What is the pressure in the container if the temperature remains constant?
Using the ideal gas law (PV = nRT) and assuming the number of moles and temperature remain constant, the initial and final pressures can be related by P1V1 = P2V2. Plugging in the values, the final pressure in the container after expansion to 12.0 L is 68.3 kPa.
Why would the pressure of a sample of gas at a constant volume fall mm Hg?
The pressure of a gas at constant volume can fall due to a decrease in temperature, as described by Gay-Lussac's law. When the temperature of the gas decreases, the kinetic energy of the gas molecules reduces, leading to fewer collisions with the container walls and consequently lower pressure. Additionally, if the gas is allowed to expand or if there are any leaks in the system, the pressure would also decrease.
What is isobaric process?
An isobaric process is a thermodynamic process that occurs at a constant pressure. This means that the system is allowed to exchange heat with its surroundings but the pressure remains the same throughout the process. In an isobaric process, the work done is determined by the change in volume of the system.
