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Raising the temperature of a gas will only increase the pressure if the volume is conserved, decreased, or (only sometimes) increased. The equation relating all three of these variables is:
PV = nRT, or
Pressure(in pascales) x Volume(in m3) = (number of moles of gas) x 8.3145(J/mol*K) x Temperature(in degrees Kelvin)
We can figure out the answer to your question by using some arbitrary numbers in this equation: we will say that the original Pressure is 101325 pascales (1atm), Volume is 2m3, T is 300oK, and the number of moles of gas is 81.24 moles.
This gives us the equation for the original system:
(101325 pascales)(2m3)=(8.3145J/mol*K)(81.24mol)(300oK)
Let's now increase the temperature by 50oK, to 350oK. We will also conserve the original volume, and see if the pressure increases. This gives us the new equation:
(X pascales)(2m3)=(8.3145J/mol*K)(81.24mol)(350oK).
Since both n and R are constants when considering the same system, we do not need to investigate what will happen when these two are changed (since a change in these two is practically infeasable).
If we solve for Pressure algebraically, we find that:
X pascales = (8.3145J/mol*K)(81.24mol)(350oK)/(2m3) = 118207 pascales.
Since our new pressure, 118207 pascales, is larger than the orgininal pressure, 101325 pascales, we can see that an increase in temperature results in an increase in pressure if volume is conserved.
Additionally, we can investigate what happens when the volume is decreased by 1m3 (from 2m3 to 1m3) along with an increase in temperature by 50oK, to 350oK. We will be comparing this new system to the old system already established in the previous part of this problem. This gives us an equation for the new system:
(X pascales)(1m3)=(8.3145J/mol*K)(81.24mol)(350oK)
If we solve for Pressure algebraically, we find that:
X pascales = (8.3145J/mol*K)(81.24mol)(350oK)/(1m3) = 236414 pascales.
Since our new pressure, 236414 pascales, is larger than the orgininal pressure, 101325 pascales, we can see that an increase in temperature results in an increase in pressure if volume is decreased.
But: what happens if the Volume is increased? Let's consider a situation where an increase in temperature by 50oK, to 350oK is accompanied by a decrease in volume by 1m3, from 2m3 to 3m3. This gives us the equation:
(X pascales)(3m3)=(8.3145J/mol*K)(81.24mol)(350oK)
If we solve for Pressure algebraically, we find that:
X pascales = (8.3145J/mol*K)(81.24mol)(350oK)/(3m3) = 78804 pascales.
Since our new pressure, 78804 pascales, is smaller than the orgininal pressure, 101325 pascales, we can see that an increase in temperature DOES NOT always result in an increase in pressure if volume is increased.
As a general rule, we can therefore conclude that an increase in volume does not always result in an increase in pressure if the temperature is increased. However, there are marginal situations in which this CAN happen: if, for example, the volume is increased by 0.0000001m3, along with an increase in temperature to 350oK, we find that solving for the Pressure gives us a value of 118207 pascales, which is larger than our original pressure, 101325 pascales. So, we can see that an increase in temperature CAN SOMETIMES result in an increase in pressure if volume is increased.
An increase in volume only increases pressure in a system if the increase in volume is significantly small when compared to the increase in temperature.
What else can I help you with?
When does raising the temperature of gas increase its pressure?
Raising the temperature of a gas increases its pressure when the volume of the gas is kept constant. This is described by the ideal gas law, which states that pressure is directly proportional to temperature when volume is constant. When the temperature of a gas is increased, the average kinetic energy of the gas particles increases, leading to more frequent and forceful collisions with the walls of the container, resulting in higher pressure.
Raising temperature of a gas fixed volume container will change?
The pressure of the gas inside the container will increase due to the increased kinetic energy of the gas molecules. This is described by the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
How will a pressure increase affect a gaseous system?
According to Boyle's Law of Pressure-Volume Relationship, an increase in the pressure of a gas will decrease it's volume. And according to Charles's Law of Temperature-Pressure Relationship, an increase in pressure causes an increase in temperature.
When the temperature of a gas is constant will the volume increase or decrease as the pressure decreases?
When the temperature of a gas is constant and the pressure decreases, the volume will increase. This is described by Boyle's Law, which states that at constant temperature, the pressure and volume of a gas are inversely proportional to each other.
As the temperature of a fixed volume of a gas increases the pressure will?
decrease
Raising the temperature of a gas will increase its pressure IF the volume of the gas?
Boyle's law states that the volume of a gas is inversely proportional to its pressure if the
What raising the temperature of a gas will increase its pressure if the volume of the gas?
Boyle's law states that the volume of a gas is inversely proportional to its pressure if the
What will raising the temperature of a gas will increase its pressure if the volume of the gas?
Boyle's law states that the volume of a gas is inversely proportional to its pressure if the
When does raising the temperature of gas increase its pressure?
Raising the temperature of a gas increases its pressure when the volume of the gas is kept constant. This is described by the ideal gas law, which states that pressure is directly proportional to temperature when volume is constant. When the temperature of a gas is increased, the average kinetic energy of the gas particles increases, leading to more frequent and forceful collisions with the walls of the container, resulting in higher pressure.
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.
When does raising the temperature of a gas increase the pressure?
This is possible in a closed system.
Raising temperature of a gas fixed volume container will change?
The pressure of the gas inside the container will increase due to the increased kinetic energy of the gas molecules. This is described by the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
What of the following would increase the pressure of a gas in a container?
The pressure of a gas in a container can be increased by raising the temperature of the gas, which causes the molecules to move faster and collide with the container walls more frequently and with greater force. Additionally, reducing the volume of the container while keeping the temperature constant will also increase the pressure, as the gas molecules have less space to move and collide more often. Lastly, adding more gas molecules to the container will increase the number of collisions with the walls, thereby raising the pressure.
What happens to the pressure of gas if the temperature of the gas is increased?
The pressure of a gas increases with an increase in temperature.
What happens to the pressure of the gas if the temperature of the gas is increased?
The pressure of a gas increases with an increase in temperature.
What effect does raising the temperature of a gas have on its pressure if the volume of the gas and the number of particles are kept constant?
Raising the temperature of a gas will increase its pressure, following the ideal gas law (PV = nRT). As temperature increases, the average kinetic energy of the gas particles also increases, leading to more frequent and forceful collisions with the walls of the container, resulting in higher pressure.
Does temperature of a gas increase or decrease under pressure?
When pressure on a gas increases, its temperature also increases. This relationship is described by the ideal gas law (PV = nRT), showing that an increase in pressure leads to an increase in temperature to maintain the same volume and number of moles of gas.
