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First find moles hydrogen gas.
20 grams H2 (1 mole H2/2.016 grams)
= 9.921 moles H2
Now, the ideal gas equation.
PV = nRT
(1 atm)(volume L) = (9.921 moles H2)(0.08206 L*atm/mol*K)(298.15 K)
Volume of hydrogen gas = 243 Liters
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What else can I help you with?
The volume of 1mole of hydrogen bromide at STP is 22.4 liters The gram-formula mass of hydrogen bromide is 80.9 grams per mole What is the density of hydrogen bromide at STP?
The molar volume of a gas at STP is 22.4 liters/mol. The molar mass of hydrogen bromide is 80.9 g/mol. Therefore, the density of hydrogen bromide at STP is 80.9 g/mol / 22.4 L/mol = 3.61 g/L.
What is the volume of 2 moles of Hydrogen?
The volume of hydrogen is 97, 86 L.
How many liters of hydrogen gas are needed to react with CS2 to produce 2.5L of CH4 at STP?
The balanced equation for the reaction between hydrogen gas (H2) and carbon disulfide (CS2) to produce methane (CH4) is: 4H2 + CS2 → 4H2S + CH4. This means that for every 4 moles of hydrogen gas, 1 mole of methane is produced. Since 1 mole of any gas at STP occupies 22.4 liters, you would need 5.6 liters of hydrogen gas to produce 2.5 liters of methane.
Identify the limiting and excess reagents when 25 liters of nitrogen reacts with 25 Liters of hydrogen.How many liters of ammonia gas are formed in this reaction?
# This is a stoichiometry problem and requires a balanced chemical equation. N2 + 3 H2 ----> 2 NH3 If we assume that this reaction occurs at STP, then the number of moles of any gas at STP is equal to the volume (in litres) divided by 22.4 This will get you started.1500ml
How many moles of sulfur dioxide gas ocupy a volume of 444 liters at stp?
Assuming it acts as an ideal gas then you use the equation PV=nRT where P=pressure (101.325 kPa at STP) V = volume 444 L (given) n = number of mols R = gas constant, 8.314472 L kPa K-1mol-1 T = temperature 273.15 K at STP I got 19.81 mols.
What is molar volume of hydrogen at stp?
The molar volume of hydrogen gas at STP (Standard Temperature and Pressure) is 22.4 liters per mole.
The volume of 1mole of hydrogen bromide at STP is 22.4 liters The gram-formula mass of hydrogen bromide is 80.9 grams per mole What is the density of hydrogen bromide at STP?
The molar volume of a gas at STP is 22.4 liters/mol. The molar mass of hydrogen bromide is 80.9 g/mol. Therefore, the density of hydrogen bromide at STP is 80.9 g/mol / 22.4 L/mol = 3.61 g/L.
How many liters of hydrogen gas at STP can be produced with 645 grams of baking soda?
To find the volume of hydrogen gas produced, we first need to convert the mass of baking soda (645g) to moles. Then, using the balanced chemical equation for the reaction, we can determine the moles of hydrogen gas produced. Finally, using the ideal gas law at STP, we can convert the moles of hydrogen gas to liters.
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.
What sample at STP has the same number of molecules as 5 liters of NO2 at STP?
At STP, 1 mole of any ideal gas occupies 22.4 liters. Therefore, 5 liters of NO2 at STP will represent 0.22 moles (5/22.4), and this is the case for any other ideal gas. So, the answer is that 5 liter of ANY ideal gas will have the same number of molecules as 5 liters of NO2.
How many liters are in 5.4x1024 molecules of nitric oxide at STP?
Using the ideal gas law (PV = nRT), we can calculate the volume of gas at STP. First, we need to convert the number of molecules to moles by dividing by Avogadro's number. Then, we can use the volume of 1 mole of gas at STP, which is 22.4 liters. Calculate V = (5.4x10^24 / 6.022x10^23) * 22.4 to find the volume in liters.
What is the volume of 2 moles of Hydrogen?
The volume of hydrogen is 97, 86 L.
How many atoms of hydrogen are in 67.2 l of h2 at stp?
At STP (Standard Temperature and Pressure), the volume of 1 mole of any gas is 22.4 liters. Since hydrogen gas exists as H2 molecules, 67.2 liters of hydrogen gas at STP contains 3 moles of H2 molecules. Since each H2 molecule contains 2 hydrogen atoms, there are 6 moles of hydrogen atoms, which is equivalent to 6 x 6.022 x 10^23 atoms of hydrogen.
Calculate the number of moles in 15 liters of oxygen at STP?
At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. Therefore, 15 liters of oxygen at STP would be equivalent to 15/22.4 = 0.67 moles.
How many liters of hydrogen gas are needed to react with CS2 to produce 2.5L of CH4 at STP?
The balanced equation for the reaction between hydrogen gas (H2) and carbon disulfide (CS2) to produce methane (CH4) is: 4H2 + CS2 → 4H2S + CH4. This means that for every 4 moles of hydrogen gas, 1 mole of methane is produced. Since 1 mole of any gas at STP occupies 22.4 liters, you would need 5.6 liters of hydrogen gas to produce 2.5 liters of methane.
How do you calculate the number of liters of 3.30 moles of helium at stp?
1 mole occupies 22.414 liters So, 3.30 moles will occupy 73.966 liters.
How many hydrogen molecules are in 31.8 L H2(g) at STP?
To find the number of hydrogen molecules, first calculate the number of moles in 31.8 L of H2 at STP using the ideal gas law. Then use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
