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What is the volume occupied by 56 grams of water vapor at a temperature of 274 kelvin and a pressure of 108 kPa?
n = 56 g/ (18.0 g/mole) = 3.11 moles water.
P = (108 kPa) / (101.325 kPa/ATM) = 1.065877 ATM
R = universal gas constant = 0.0820574587L · ATM · K-1 · mol-1
V = nRT/P = (3.11 mol) * (0.082057L · ATM · K-1 · mol-1) * (274 K) / 1.06588 ATM
= 65. 6 L
Note: a mole of water vapor (H2O) is 18.0 grams, since it has an molar mass of 18. Oxygen has a molar mass of 16.0, and the two hydrogen atoms each have a molar mass of 1.0.
What else can I help you with?
When using Charles's law temperature must be on the?
Temperature must be in Kelvin when using Charles's law, as it is a gas law that states that the volume of a gas is directly proportional to its absolute temperature when pressure and amount of gas are constant.
What volume is occupied of 2.4 moles of chlorine?
The volume that 2.4 moles of chlorine gas would occupy depends on the temperature and pressure of the gas, according to the ideal gas law (PV = nRT). At standard temperature and pressure (STP), which is 0°C and 1 atm pressure, 2.4 moles of chlorine gas would occupy approximately 53.75 liters.
If 20.0 of gas has a volume of 4.00 and a pressure of 6.00 what is its temperature in degrees Celsius?
136 C From Ideal gas equation: PV = nRT where V is volume, P is pressure and T temperature. n is moles and R is Universal gas constant. Moles of N2 = 20.0 g * (1 mol / 28.013 g) = 0.714 mol Volume, V = 4.00 L Pressure, P = 6.00 atm T = PV/nR = 6.00 atm * 4.00 L / (0.714 mol * 0.0821 Latm/mol K) = 410 K Then temperature in C is 409 - 273 = 137 C
What will happen to the volume of one liter of air if you increase its temperature from 25 degrees celsius to body temperature?
The volume of one liter of air will increase because as the temperature increases, the air molecules gain energy and move faster, causing the air to expand. This relationship is described by Charles's Law, which states that the volume of a gas is directly proportional to its temperature in Kelvin, assuming constant pressure and amount of gas.
A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37 degrees Celsius How many moles of nitrogen are in the container?
To calculate the number of moles of nitrogen gas in the container, you can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Convert the pressure to atm, the volume to L, and the temperature to Kelvin. Then plug in the values and solve for n.
If you have three liters of gas at a certain kelvin temperature and a certain pressure. The kelvin temperature triples and the pressure stays the same. What is the gas volume?
According to Charles's Law, the volume of a gas is directly proportional to its Kelvin temperature when pressure is constant. Therefore, if the Kelvin temperature triples, the gas volume will also triple, so the gas volume will be 9 liters.
What happens to the pressure of gas when the volume is doubled and no change in Kelvin temperature?
According to Boyle's Law, when the volume of a gas is doubled with no change in Kelvin temperature, the pressure of the gas will be halved. This is because pressure and volume are inversely proportional in a gas at constant temperature.
What happens to pressure when the temperature and volume is halved?
if kelvin temp is halved, the volume is halved if pressure is constant.
What is it when the volume of a gas increases and its pressure decreases?
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
What volume is occupied of 0.48 moles of hydrogen?
The volume of a gas depends on its pressure, temperature, and volume according to the ideal gas law PV = nRT. Without knowing the pressure, temperature, or container size, it's not possible to determine the volume occupied by the 0.48 moles of hydrogen.
What is volume occupied by a mole of an ideal gas if the pressure is 626mmHg and the temperature is 25.0C?
The volume occupied by a mole of an ideal gas can be calculated using the ideal gas law equation: PV = nRT. Convert the pressure to atm (1 atm = 760 mmHg), and the temperature to Kelvin (25.0°C = 298 K). Then substitute the values into the equation and solve for volume (V).
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.
Gay lussac's law relates temperature of a gas to its?
Gay-Lussac's law relates the pressure of a gas to its temperature, under constant volume and amount of gas. It states that the pressure of a gas is directly proportional to its temperature in kelvin.
When the pressure on a gas increases at constant temperature its volume?
decreases
What are the most common units of pressure volume and temperature?
pressure -- Torr which is equivalent to mmHg, Pascals or kPa, atmospheres, psi, inches Hg Volume -- usually liters Temperature -- Kelvin or Celsius which must be converted to Kelvin to be used in any gas law equations
What is it called when the volume of a gas increases and the pressure decreases?
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
What is the relationship between the kelvin temperature and the pressure of gas?
Increased temperature = increased volume of gas The above answer is non-sense. The pressure could increase with temperature and actually yield a smaller volume... here ya go: The ideal gas law is: PV = nRT, where P = pressure, V = volume, n= number of moles, R = ideal gas constant, T = Temperature in K
