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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
17 l
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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?
25 ml. The volume would not change. Now pressure on the other hand...
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?
468ml
What is the volume of 85.1g of acetone?
The volume (at 20 degrees celsius and a pressure of 1 atmosphere) is 107.7mL. Both changes in temperature or pressure will change the answer.
What is the new volume of a 3.0L sample of nitrogen gas that is heated from 75 degrees Celsius to 150 degrees Celsius?
Vf = 3.0/75 (150) = 6
If a certain amount of gas fills a 1.0 liter container and exerts a pressure on the walls of 2.0 Nm2 at 20 degrees celsius what would the pressure theoretically be at absolute zero?
Zero. PV = nRT. T = 0, so nRT = 0, and thus PV must be zero also. Since we know the volume is not zero, the pressure must be zero.
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.
A sample of Xenon gas at 20degree Celsius and 0.570 ATM is cooled to a pressure of 0.100 ATM If the volume remains constant What is the final Celsius temperature?
Using the ideal gas law, we can calculate the final temperature of the Xenon gas. Since the volume remains constant, we can use the combined gas law (P₁/T₁ = P₂/T₂) to solve for the final temperature. Rearranging the equation gives T₂ = (P₂ / P₁) * T₁. Plugging in the values, we get T₂ = (0.100 / 0.570) * 20 degrees Celsius = 3.51 degrees Celsius.
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?
25 ml. The volume would not change. Now pressure on the other hand...
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?
468ml
What is the volume of a 24.7 mol gas sample that has a pressure of 999 ATM at 305 K?
Using the ideal gas law, V = (nRT)/P where n is the number of moles, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure. Plug in the values: V = (24.7 mol * 0.0821 Latm/molK * 305 K) / 999 ATM = 6.45 L.
When a fixed sample of gas increases in volume?
Decrease its pressure.
Why volume of water exerts greater pressure than volume of air?
Water is denser than air, meaning there are more water molecules in a given volume than air molecules. This greater density of water results in more molecules colliding with the surface, creating higher pressure. Additionally, water is less compressible than air, so changes in volume have a more pronounced impact on pressure.
What is the volume of 85.1g of acetone?
The volume (at 20 degrees celsius and a pressure of 1 atmosphere) is 107.7mL. Both changes in temperature or pressure will change the answer.
How many moles of carbon dioxide are there in a 50.0 dm3 sample of the gas at a pressure of 100.0 kPa and a temperature of 50 degrees celsius?
To find the moles of carbon dioxide, we need to use the ideal gas law equation: PV = nRT. First, convert the temperature to Kelvin by adding 273.15 (50°C + 273.15 = 323.15 K). Then, plug in the values for P, V, R, and T to solve for n (moles). After calculations, you will find the number of moles of carbon dioxide in the given sample.
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?
the 30L water vapor sample is a gas gases exert pressure on their surroundings thus taking on the shape of their containers the gas is under 1 ATM of pressure so it exerts pressure in return and the volume becomes 30L when the presures are equal if the temperature were to decrease to room temperature, the water vapor would condense to a liquid and the volume would decrease liquids have a volume but no definite shape while gases have neither a definite volume or shape
At 7.0C the volume of a gas is 49 mL At the same pressure its volume is 74 mL at what temperature?
Using the ideal gas law, V1/T1 = V2/T2, where V is volume and T is temperature, we can set up an equation to solve for the final temperature. Plugging in the given values, we get 49mL/7°C = 74mL/T2. Solving for T2 gives approximately 10.9°C.
What is the new volume of a 3.0L sample of nitrogen gas that is heated from 75 degrees Celsius to 150 degrees Celsius?
Vf = 3.0/75 (150) = 6
