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What is the volume of 19.87 mol of ammonium chloride NHÁCl at STP?
To find the volume of 19.87 mol of NH₄Cl at STP (standard temperature and pressure), we can use the ideal gas law. At STP, 1 mol of gas occupies 22.4 L. Therefore, 19.87 mol of NH₄Cl will occupy 19.87 mol x 22.4 L/mol = 445.888 L.
How do you calculate the volume in liters of 1.50 mol Cl2 at stp?
To calculate the volume of a gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. At STP, the pressure is 1 atm, the temperature is 273 K, and the molar volume of an ideal gas is 22.4 L/mol. Plugging in the values, you can calculate the volume of 1.50 mol of Cl2 at STP.
What is the volume of oxygen that will be used by 12g of Mg to be completely converted into MgO?
The balanced chemical equation for the reaction is 2Mg + O2 -> 2MgO. This means that 1 mol of Mg will react with 0.5 mol of O2 to form 1 mol of MgO. The molar mass of Mg is 24 g/mol and MgO is 40 g/mol. Therefore, 12 g of Mg will require 3 mol of O2 (3 * 32 g) for complete conversion to MgO.
How a box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0 and degC. statements is true?
This statement is true. According to the ideal gas law, at 0°C and 1 atm pressure, 1 mol of any ideal gas occupies 22.4 L of volume. Therefore, 1.0 mol of nitrogen would occupy 22.4 L and 2.0 mol of hydrogen would occupy 44.8 L in a 22.4 L box.
What is the volume of 2.22 mol of o2 at STP?
The volume of 1 mol of gas at STP (standard temperature and pressure) is 22.4 L. Therefore, the volume of 2.22 mol of O2 at STP would be 2.22 mol x 22.4 L/mol = 49.7 L.
What does avagadros law say about a gas at STP?
1 mol of any gas has a volume of 22.4 L at STP
What volume will 1.50 mol of C2H4 gas occupy at STP?
At STP (Standard Temperature and Pressure), 1 mole of gas occupies 22.4 liters. Therefore, 1.50 mol of C2H4 gas would occupy 1.50 x 22.4 = 33.6 liters of volume at STP.
What is the volume of 19.87 mol of ammonium chloride NHÁCl at STP?
To find the volume of 19.87 mol of NH₄Cl at STP (standard temperature and pressure), we can use the ideal gas law. At STP, 1 mol of gas occupies 22.4 L. Therefore, 19.87 mol of NH₄Cl will occupy 19.87 mol x 22.4 L/mol = 445.888 L.
How do you calculate the volume in liters of 1.50 mol Cl2 at stp?
To calculate the volume of a gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. At STP, the pressure is 1 atm, the temperature is 273 K, and the molar volume of an ideal gas is 22.4 L/mol. Plugging in the values, you can calculate the volume of 1.50 mol of Cl2 at STP.
What is the volume of oxygen that will be used by 12g of Mg to be completely converted into MgO?
The balanced chemical equation for the reaction is 2Mg + O2 -> 2MgO. This means that 1 mol of Mg will react with 0.5 mol of O2 to form 1 mol of MgO. The molar mass of Mg is 24 g/mol and MgO is 40 g/mol. Therefore, 12 g of Mg will require 3 mol of O2 (3 * 32 g) for complete conversion to MgO.
How a box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0 and degC. statements is true?
This statement is true. According to the ideal gas law, at 0°C and 1 atm pressure, 1 mol of any ideal gas occupies 22.4 L of volume. Therefore, 1.0 mol of nitrogen would occupy 22.4 L and 2.0 mol of hydrogen would occupy 44.8 L in a 22.4 L box.
What is the volume at 273 K and 1 Bar?
At 273 K (0°C) and 1 bar pressure, the molar volume of an ideal gas is approximately 24.79 L/mol. This value represents the volume occupied by one mole of the gas under these conditions.
How many liters of oxygen gas are present in 11.3 grams of oxygen gas?
To find the number of liters of oxygen gas in 11.3 grams, you need to convert the grams to moles using the molar mass of oxygen (16 g/mol). Then, you can use the ideal gas law to find the volume of gas at standard temperature and pressure (STP), which is 1 mole of gas occupying 22.4 liters at 0 degrees Celsius and 1 atm pressure.
What is the volume of 12g of NO2 at STP?
At STP, 1 mole of an ideal gas occupies 22.4 liters. 0.335 mol x 22.4 L = 7.50 L .................. 1 mol
A mixture of gases contains 0.25 mol oxygen gas 0.75 mol nitrogen gas and 1.50 mol carbon dioxide gas at STP The mole fraction of oxygen gas in this mixture is?
At STP (Standard Temperature and Pressure), the volume occupied by 1 mol of any gas is 22.4 L. Thus, 0.25 mol of oxygen gas occupies (0.25 mol) * (22.4 L/mol) = 5.6 L in the mixture. The total volume of the gas mixture can be found as the sum of the individual volumes of oxygen, nitrogen, and carbon dioxide. Then, the mole fraction of oxygen gas is the moles of oxygen gas divided by the total moles of all gases in the mixture.
What is the volumes of gas molecules relative to the total gas volume?
The volume of gas molecules is negligible compared to the total gas volume. Gas molecules themselves occupy a very small fraction of the total volume of the gas, with the majority of the volume being empty space between the molecules.
What is the volume of 2.22 mol of o2 at STP?
The volume of 1 mol of gas at STP (standard temperature and pressure) is 22.4 L. Therefore, the volume of 2.22 mol of O2 at STP would be 2.22 mol x 22.4 L/mol = 49.7 L.
