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What would be the mass in grams of 186 mL of nitrogen gas?
To find the mass of nitrogen gas, you need to know the density of nitrogen gas at the given conditions (typically at STP - standard temperature and pressure). The density of nitrogen at STP is about 1.25 g/L. You can use this value to calculate the mass by multiplying the density by the volume given in milliliters.
What is 10cm3 in nitrogen?
10 cm³ of nitrogen refers to a volume of nitrogen gas measured at standard temperature and pressure (STP). At STP, 1 mole of any gas occupies approximately 22.4 liters (or 22,400 cm³). Therefore, 10 cm³ of nitrogen is a small fraction of a mole, specifically about 0.000446 moles of nitrogen gas.
What is the atomic mass number for nitrogen?
The atomic weight is14.00674
How do you find liters of hydrogen and nitrogen gas required to produce 532 liters of ammonia using 3H2 g plus N2 g--- 2NH3 g?
Let x = hydrogen gas 532 / 2 = x / 3 .... x = 798L Let y = nitrogen gas 532 / 2 = y / 1 .... y = 266L
How many grams of methane gas CH4 are contained in a volume of 144 liters at STP?
At STP (standard temperature and pressure), one mole of any gas occupies 22.4 liters. This means that 144 liters of methane gas contain 144/22.4 moles of CH4. Using the molar mass of CH4 (16 g/mol), you can calculate the mass of methane gas in grams.
If 6 liters of hydrogen gas are used how many liters of nitrogen gas will be needed for the above reaction at standard temperature and pressure?
Assuming you are referring to the reaction of hydrogen and nitrogen to form ammonia, the balanced equation is: 3H2 + N2 → 2NH3 From the equation, 3 liters of hydrogen gas react with 1 liter of nitrogen gas. Therefore, if 6 liters of hydrogen gas are used, you would need 2 liters of nitrogen gas.
If 6 liters of hydrogen gas are used how many liters of nitrogen gas will be needed for the above reaction at STP?
For the reaction N₂ + 3H₂ → 2NH₃, the mole ratio of hydrogen gas to nitrogen gas is 3:1. Since 6 liters of hydrogen gas is used, you would need 2 liters of nitrogen gas at STP for this reaction according to the stoichiometry of the reaction.
How many liters of hydrogen gas are in gaseous ammonia?
There are no liters of hydrogen gas in gaseous ammonia. Ammonia (NH3) consists of nitrogen and hydrogen atoms, but the hydrogen is chemically bonded to the nitrogen.
What Maximum percentage of nitrogen by mass?
The maximum percentage of nitrogen by mass is about 78.08%, which is the composition of nitrogen gas (N2) in the atmosphere.
When 1 liter of nitrogen gas reacts with 3 liters of hydrogen gas at constant temperature and pressure how many liters of ammonia gas will be produced?
When 1 liter of nitrogen gas reacts with 3 liters of hydrogen gas, they will react to produce 2 liters of ammonia gas. This follows the balanced chemical equation: N2 + 3H2 → 2NH3. Each mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.
What is the volume of 1 mole of nitrogen?
The molar volume of nitrogen gas at standard temperature and pressure (STP) is approximately 22.4 liters. This means that 1 mole of nitrogen gas occupies 22.4 liters of space under these conditions.
What is the mass in g of 186 ml of nitrogen gas?
To find the mass of nitrogen gas, we need to know the density of nitrogen gas at a given temperature and pressure. The density of nitrogen gas at standard conditions (0°C and 1 atm) is approximately 1.25 g/L. Therefore, the mass of 186 ml (0.186 L) of nitrogen gas would be around 0.2325 grams.
What is the mass of 1 Mole of diatomic nitrogen gas?
The molar mass of diatomic nitrogen (N2) is approximately 28.02 g/mol. Therefore, the mass of one mole of diatomic nitrogen gas is 28.02 grams.
What is the mole for 11.2 liters of two atoms of nitrogen?
The number of moles in 11.2 liters of nitrogen gas (N2) can be calculated using the ideal gas law. Since you have two nitrogen atoms per molecule of N2, you would need to convert the volume of gas to moles using the ideal gas constant.
Gaseous ammonia is made by the following reaction n2 plus 3h 2nh3 if you start with 7 l of nitrogen gas how many liters of hydrogen are needed for a complete reaction?
According to the balanced chemical equation, for every 1 mole of nitrogen gas (N2), 3 moles of hydrogen gas (H2) are needed. Since the volume of a gas is directly proportional to the number of moles, you would need 21 liters of hydrogen gas (3 times 7 liters) to react completely with 7 liters of nitrogen gas to produce ammonia.
What is the mass of 2.50 X 104 molecules of nitrogen gas?
To calculate the mass of 2.50 x 10^4 molecules of nitrogen gas, you need to know the molecular weight of nitrogen. The molar mass of nitrogen (N2) is approximately 28.02 g/mol. Using this information, you can then calculate the mass of 2.50 x 10^4 molecules of nitrogen gas.
What would be the mass in grams of 186 mL of nitrogen gas?
To find the mass of nitrogen gas, you need to know the density of nitrogen gas at the given conditions (typically at STP - standard temperature and pressure). The density of nitrogen at STP is about 1.25 g/L. You can use this value to calculate the mass by multiplying the density by the volume given in milliliters.
