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A 0.50 mole sample of any ideal gas, including helium, will occupy 11.2 liters at standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atm pressure.
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.
The answer is 0,19 moles.
At standard temperature and pressure conditions, 1 kilogram of gaseous hydrogen would occupy a volume of about 11.1 cubic meters.
At room temperature and pressure, 125 g of CO2 will occupy approximately 44.8 liters. This is calculated using the ideal gas law, which assumes ideal gas behavior.
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.
A 0.50 mole sample of any ideal gas, including helium, will occupy 11.2 liters at standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atm pressure.
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.
The volume of gas depends on the temperature, pressure, and number of gas particles present. These factors affect the amount of space the gas particles occupy.
The answer is 0,19 moles.
The volume of 0.8 moles of a gas at Standard Temperature and Pressure (STP) is 17.6 liters. This is because at STP, one mole of any ideal gas occupies 22.4 liters.
At standard temperature and pressure conditions, 1 kilogram of gaseous hydrogen would occupy a volume of about 11.1 cubic meters.
22g of CO2 at STP (standard temperature and pressure) is equivalent to 1 mole. The volume occupied by 1 mole of any gas at STP is approximately 22.4 liters.
At room temperature and pressure, 125 g of CO2 will occupy approximately 44.8 liters. This is calculated using the ideal gas law, which assumes ideal gas behavior.
At standard atmospheric pressure and temperature, 1 kg of air occupies about 0.831 m³.
10 mg of 'standard' pure water, at standard temperature and pressure, occupy 0.01 mL of space.
When the temperature of a gas is increased at constant pressure, its volume also increases. This relationship is described by Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant. As the gas molecules gain energy with increased temperature, they move more quickly and occupy a larger volume.