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How does the volume of a gas vary?
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.
What is the unit of measurement measures atmospheric pressure?
ATM
What is the pressure of a fixed volume of hydrogen gas at 34.9C if it has a pressure of 1.33 ATM at 15.0C?
2.79 ATM
What is the final pressure of a system (ATM) that has the volume increased from 0.75 L to 3.1L with an initial pressure of 1.25 ATM?
1.1
0.783 g of hydrogen gas is placed in an container of volume 657 mL at a temperature of 342 K What is the pressure in ATM?
Using the Ideal Gas Law (PV = nRT), you can calculate the pressure of the hydrogen gas. First, convert the mass of hydrogen to moles using the molar mass of hydrogen. Once you have moles of hydrogen, you can calculate the pressure given the volume, temperature, and the gas constant (0.0821 Latm/molK).
An oxygen cylinder used for breathing has a volume of 5.5 L at 78 ATM pressure. What is the volume of the same amount of oxygen at the same temperature if the pressure is 1.0 ATM?
To find the volume of oxygen at 1.0 ATM pressure, we can use Boyle's Law, which states that pressure and volume are inversely proportional at constant temperature (P1V1 = P2V2). Given P1 = 78 ATM, V1 = 5.5 L, P2 = 1.0 ATM, we can rearrange the equation to find V2: V2 = (P1V1) / P2 = (78 ATM * 5.5 L) / 1.0 ATM = 429 L. Thus, the volume of oxygen at 1.0 ATM is 429 liters.
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 change in pressure would result in the volume of gas increasing A 2 ATM to 3 ATM B 3 ATM to 4 ATM C 4 ATM to 1 ATM D 1 ATM to 3 ATM?
A. An increase in pressure from 2 ATM to 3 ATM will result in a decrease in volume of gas. B. An increase in pressure from 3 ATM to 4 ATM will result in a decrease in volume of gas. C. A decrease in pressure from 4 ATM to 1 ATM will result in an increase in volume of gas. D. An increase in pressure from 1 ATM to 3 ATM will result in a decrease in volume of gas.
What determines a gas's of volume?
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the volume of 22.4 liters.
22.41 L is the volume of 1 mol of gas at?
STP (standard temperature and pressure), which is 0 degrees Celsius and 1 atm pressure.
How does the volume of a gas vary?
Pressure and temperature. As pressure increases, volume decreases; as temperature increases, volume increases with it. At standard temperature and pressure (1 atm, 273 degrees Kelvin), one mole of a gas (6.022 x 1023 particles) has the 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.
A 5.0 liter tank of oxygen gas is at a pressure of 3 ATM What volume of oxygen will be available if the oxygen is used at a standard pressure?
If the oxygen is used at standard pressure (1 ATM), the volume of oxygen available will be 5.0 liters. This is because the volume of a gas is directly proportional to its pressure when the temperature remains constant, according to Boyle's Law (P1V1 = P2V2).
What is the volume of 3.7L of gas after its pressure is increased from 2.5 ATM to 4.5 ATM?
V1 = 4L, P1 = 2.07 atm, P2= ?, V2 = 2.5L We will use following equation to solve this problem: P1V1/T1 = P2V2/T2 Assume Temperature is constant (as nothing is mentioned about temperature in our problem) so our new equation will be P1V1 = P2V2 Plugging in the values (2.07 atm)(4L) = P2(2.5L) so P2 = (2.07atm) (4L)/(2.5L) (Rearranging the terms) P2 = 3.312 atm Pressure and volume are inversely related at constant temperature.
What is the unit of measurement measures atmospheric pressure?
ATM
If i have 5.6liters of gas in a piston at a pressure of 1.5 ATM and compress the gas volume is 4.8L what will the new pressure be?
To find the new pressure, we can use Boyle's Law, which states that pressure and volume are inversely proportional at constant temperature. By applying the formula P1V1 = P2V2, where P1 = 1.5 ATM, V1 = 5.6 L, and V2 = 4.8 L, we can solve for P2. Thus, the new pressure would be 1.75 ATM.
What is the pressure of a fixed volume of hydrogen gas at 34.9C if it has a pressure of 1.33 ATM at 15.0C?
2.79 ATM
