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A 30 L sample of gas exerts 200 mm Hg pressure at 10 Celsius What volume does the gas have at 300 mm Hg and 25 Celsius?
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∙ 10y ago
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A 25 ml sample of gas in enclosed in a gas tight syringe at 22 degrees Celsius if the syringe is immersed in an ice bath at 0 degrees Celsius what is the new gas volume?
Using the ideal gas law, (P1V1)/T1 = (P2V2)/T2, where P is pressure, V is volume, and T is temperature. Assuming constant pressure, the new gas volume at 0 degrees Celsius can be calculated using the initial volume (25 ml) and temperatures (22 degrees Celsius and 0 degrees Celsius). By plugging in the values and rearranging the equation, you can find the new gas volume in the syringe after immersing it in the ice bath.
What is the new volume of a 3.0L sample of nitrogen gas that is heated from 75 degrees Celsius to 150 degrees Celsius?
To find the new volume of the sample of nitrogen gas, you would need to use the ideal gas law equation, which is PV = nRT. Given that temperature and pressure have changed, you should calculate the new volume using the new temperature. Remember to convert the temperatures to Kelvin (273 + degrees Celsius) before plugging them into the equation.
What is the volume 1 g or water at 4 degrees celsius and a pressure at 1 ATM?
The volume of 1 g of water at 4 degrees Celsius and 1 ATM pressure is approximately 1.002 mL.
What are the Kinetic Molecular Theory effects on the pressure and volume of the gas sample?
According to the Kinetic Molecular Theory, pressure is the result of gas molecules colliding with the walls of the container. As the volume of the gas sample decreases, the frequency of collisions increases, leading to an increase in pressure. Conversely, as the volume increases, the frequency of collisions decreases, leading to a decrease in pressure.
Under what sets of condition will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
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.
What will be the new volume of a 1.75 L sample cooled from 25 degrees celsius to 0 degrees celsius at constant pressure?
The volume of the sample will decrease as it cools down due to thermal contraction. To calculate the new volume, you can use the formula for thermal expansion: V2 = V1 * (1 + β*(T2 - T1)), where V1 = 1.75 L, T1 = 25°C, T2 = 0°C, and β is the coefficient of volume expansion for the substance at constant pressure.
A 25 ml sample of gas in enclosed in a gas tight syringe at 22 degrees Celsius if the syringe is immersed in an ice bath at 0 degrees Celsius what is the new gas volume?
Using the ideal gas law, (P1V1)/T1 = (P2V2)/T2, where P is pressure, V is volume, and T is temperature. Assuming constant pressure, the new gas volume at 0 degrees Celsius can be calculated using the initial volume (25 ml) and temperatures (22 degrees Celsius and 0 degrees Celsius). By plugging in the values and rearranging the equation, you can find the new gas volume in the syringe after immersing it in the ice bath.
What is the volume of a quantity of gas at 152 degrees celsius if its volume is 262ml at -35.0 degrees celsius the pressure remains constant?
To find the volume of the gas at 152°C, you can use the Charles's Law equation, V1/T1 = V2/T2, where V1 is the initial volume (262 mL), T1 is the initial temperature (-35.0°C), V2 is the final volume (unknown), and T2 is the final temperature (152°C). Plug in the values and solve for V2 to find the volume of the gas at 152°C.
When a fixed sample of gas increases in volume?
When a fixed sample of gas increases in volume, its pressure decreases because the gas particles have more space to move around, resulting in fewer collisions with the container walls. The temperature of the gas typically remains constant.
Why is water a liquid at room temperature with a molar volume of 18mL and at 105 degrees C and 1 ATM pressure it is a gas with a molar volume of 30L?
At room temperature, water molecules have enough energy to overcome attractive forces and stay in a liquid state. When heated to 105 degrees C, the increased temperature causes water molecules to gain more kinetic energy, leading to increased intermolecular distances and resulting in water transitioning into a gas state with a higher molar volume. The difference in molar volume between the liquid and gas states of water at these temperatures is mainly due to the change in intermolecular distances and the expansion of the gas phase.
What is the new volume of a 3.0L sample of nitrogen gas that is heated from 75 degrees Celsius to 150 degrees Celsius?
To find the new volume of the sample of nitrogen gas, you would need to use the ideal gas law equation, which is PV = nRT. Given that temperature and pressure have changed, you should calculate the new volume using the new temperature. Remember to convert the temperatures to Kelvin (273 + degrees Celsius) before plugging them into the equation.
A gas sample is held at constant temperature. What happens to the pressure of the sample if the volume is doubled and the number of molecules is doubled?
If the volume is doubled and the number of molecules is doubled while the temperature is held constant, the pressure of the gas sample will remain the same. This is because both the volume and the number of molecules increased by the same factor, resulting in no net change in pressure according to the ideal gas law.
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.
Under what sets of condition will a 0.50 mole sample of helium occupy a volume of 11.2 liters?
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
What is stated by boyles law?
Boyle's Law states that the pressure of a gas is inversely proportional to its volume, when the temperature is kept constant. This means that as the volume of a gas decreases, the pressure it exerts increases, and vice versa. This relationship is described by the equation P1V1 = P2V2, where P represents pressure and V represents volume.
At 1250 mm Hg and 75 degrees Celsius the volume of a sample of ammonia gas is 6.28 L What volume would the ammonia occupy at STP?
Using the combined gas law, we can relate the initial and final conditions of the gas: P1V1/T1 = P2V2/T2. At STP (Standard Temperature and Pressure), the conditions are 1 atm and 0 degrees Celsius. Convert 1250 mm Hg to atm and 75 degrees Celsius to Kelvin. With this information, you can then calculate the final volume of the ammonia gas at STP.
