0
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 else can I help you with?
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
According to ideal gas eqation if pressure is double to initial pressure then what happens to the volume?
If the pressure is doubled according to the ideal gas equation (PV = nRT), and the other variables remain constant, then the volume would be halved. This is because pressure and volume are inversely proportional when the other variables are constant in an ideal gas.
What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change of temperature?
According to Boyle's Law, if you double the volume of a gas at constant temperature, the pressure is halved. So, the pressure would decrease to 190 mm Hg when the gas sample is expanded to 800 mL.
A sample of oxygen gas has a volume of 150 milliliters at 300k if the pressure of the sample is held constant and the temp raised to 600k the new sample will be?
Using the combined gas law (P1V1/T1 = P2V2/T2), we can calculate the new volume of the oxygen gas sample at 600K. Given P1V1/T1 = P2V2/T2, we have P1 = P2 (pressure is constant), V1 = 150 mL, T1 = 300K, and T2 = 600K. Plugging in these values, we get V2 = (P1 * V1 * T2) / (T1) = (1 * 150 * 600) / (300) = 300 mL. So, the new volume of the oxygen gas sample at 600K would be 300 milliliters.
Is the density of 10mLsample of water would be different than 5mL sample?
No, the density of water remains constant regardless of the sample size, as long as the temperature and pressure are the same. Density is defined as mass per unit volume, so both a 10 mL and a 5 mL sample of water will have the same density, which is approximately 1 g/mL at room temperature. Thus, the density does not change with the volume of the sample.
A sample of oxygen occupies 1.00 L If the temperature remains constant and the pressure on the oxygen is tripled what is the new volume?
According to Boyle's Law, at constant temperature, the pressure and volume of a gas are inversely proportional. So, if the pressure is tripled, the volume would become one-third of the original volume. Therefore, the new volume would be 0.33 L.
At a constant temperature what is the impact to volume if the pressure is increased?
Volume & pressure are inversely proportionate, if temperature stays constant volume would decrease at a factor proporionate to the increase in pressure.
What happens to volume when temperature of gas is decresd at constant pressure?
If the temperature of the gas is decreasing, then in order to maintain constant pressure, you would have to compress it in volume.
What is A sample of gas occupies 1.55L at STP What will the volume be if the pressure is increased to 50 ATM while the temperature remains constant?
Using the ideal gas law equation, we can calculate the new volume of the gas. At STP, the pressure is 1 atm, which means 50 atm is 50 times greater. So the new volume would be 1.55L / 50 = 0.031L, when the pressure is increased to 50 atm.
What happens to pressure of constant mass of a gas at constant temperature when the volume is doubled?
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
According to ideal gas eqation if pressure is double to initial pressure then what happens to the volume?
If the pressure is doubled according to the ideal gas equation (PV = nRT), and the other variables remain constant, then the volume would be halved. This is because pressure and volume are inversely proportional when the other variables are constant in an ideal gas.
A 175 mL sample of neon had its pressure changed from 75kPa to 150kPa what is its new volume if temperature is held constant?
Using the ideal gas law (PV = nRT), since the temperature is constant, the relationship between pressure and volume is inversely proportional. Therefore, if the pressure doubles from 75kPa to 150kPa, the volume will halve. The new volume would be 87.5 mL.
When the temperature of a gas stays constant and you decrease the volume what do you observe?
When the temperature of a gas is constant and the volume decreases, the pressure of the gas increases. This relationship is described by Boyle's Law, which states that pressure and volume are inversely proportional when temperature is held constant.
What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change of temperature?
According to Boyle's Law, if you double the volume of a gas at constant temperature, the pressure is halved. So, the pressure would decrease to 190 mm Hg when the gas sample is expanded to 800 mL.
Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the?
If the pressure of the ideal gas is kept constant and the volume is desired to double, the temperature must also double according to the ideal gas law: V2 = 2V1 = (2/1)×V1 when T2 = 2T1. This relationship results from the formula PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature.
A sample of At gas occupies a volume of 1.2 L at 125 C and a pressure of 1.0 atm. Determine the temperature, In degrees Celsius at which the volume of the gas would be 1.0 L at the same pressure?
A sample of Ar gas occupies a volume of 1.2 L at 125°C and a pressure of 1.0 atm. Determine the temperature, in degrees Celsius, at which the volume of the gas would be 1.0 L at the same pressure.
Under which conditions will the volume of a given sample of a gas always decrease?
The Ideal Gas Law states that PV=nRT, where P=pressure, V=volume, n=number of moles of gas, R=the relativity constant, and T=temp in Kelvin. According to this law, volume (V) varies as V=(nRT)/P. Using this, we can determine that the volume would normally increase with an increase in the number of moles and/or an increase in the temperature and/or a decrease in pressure. Therefore, we can logically determine that the volume of a gas would decrease in the instance of increasing temperature if either the number of moles of gas was decreased or the pressure was increased (to an extent where the level of volume increase by temperature change has been overcome.)
