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How many molecules are in 7.3 L of H2 at STP?
At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
How many atoms of hydrogen are in 16.2 l of h2 at stp?
Using stoichiometry, 16.2 L of H2 gas at STP equals about .7228 moles (1 L of gas at STP has a volume of 22.41 L), and there are 6.02 x 1023molecules of hydrogen in a mole, so we have (6.02 x 1023molecules/mol)(.7228 mol) = 4.35 x 1023 hydrogen molecules. There are two hydrogen atoms in each molecule, so the answer is (4.35 x 1023molecules H2)(2 H atoms/molecule) = 8.70 x 1023 H atoms in 16.2 L.
How many moles are in 10.3 L of helium gas at STP?
- molar mass: 34,08 g- density: 1,363 g/cm3Mass of H2S: 1,363 x 9,36 = 12,758 g34,08--------------------------1 mol12,758-------------------------xx = 0,374 moles
What is the no of molecules of H2 and CO2 with the same volume?
The molar volume at 1 bar and 0 0C is 22,710 980(38) L/mol; each mol contain 6,022 140 857.10e23 molecules.
How many moles of H2 gas are present in 6.0 L flask at stp?
The answer is 0,2675 moles.
How many molecules are in 7.3 L of H2 at STP?
At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
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.
How many atoms of hydrogen are in 16.2 l of h2 at stp?
Using stoichiometry, 16.2 L of H2 gas at STP equals about .7228 moles (1 L of gas at STP has a volume of 22.41 L), and there are 6.02 x 1023molecules of hydrogen in a mole, so we have (6.02 x 1023molecules/mol)(.7228 mol) = 4.35 x 1023 hydrogen molecules. There are two hydrogen atoms in each molecule, so the answer is (4.35 x 1023molecules H2)(2 H atoms/molecule) = 8.70 x 1023 H atoms in 16.2 L.
How many liters of hydrogen gas are needed to react with CS2 to produce 2.50 L of CH4 at STP?
Since the reaction is balanced, we can use the stoichiometry to find the volume of hydrogen gas needed. According to the reaction equation: 1 mol of CS2 reacts with 4 mol of H2 to produce 1 mol of CH4. So, 2.50 L of CH4 will need 2.50 mol of H2. At STP, 1 mol of any gas occupies 22.4 L, thus 2.50 mol of H2 will be 56 L.
How many molecules of H2(g) are there in a 21.25 gram sample?
To calculate the number of molecules, you first need to determine the number of moles of H2 in the 21.25 gram sample using the molar mass of H2 (2 grams/mol). Then, use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
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.
How many moles are in 10.3 L of helium gas at STP?
- molar mass: 34,08 g- density: 1,363 g/cm3Mass of H2S: 1,363 x 9,36 = 12,758 g34,08--------------------------1 mol12,758-------------------------xx = 0,374 moles
ANSWERED How many g of potassium must react with H20 to produce 1.60 L of H2 at STP according to the following equation?
Given the reaction 2K + 2H2O -> 2KOH + H2, we can see that 2 moles of potassium react to produce 1 mole of hydrogen gas. At STP, 1 mole of any gas occupies 22.4 L. Therefore, for 1.6 L of hydrogen gas, 2 moles of potassium are needed, which is approximately 155 g of potassium.
How many moles of NH3 are produced when 1.2 mol of H2 reacts?
The balanced chemical equation for the reaction between H2 and NH3 is: 3H2 + N2 → 2NH3 From the equation, we can see that 3 moles of H2 produce 2 moles of NH3. Therefore, when 1.2 moles of H2 react, we can calculate the moles of NH3 produced as: 1.2 mol H2 * (2 mol NH3 / 3 mol H2) = 0.8 mol NH3.
What is the no of molecules of H2 and CO2 with the same volume?
The molar volume at 1 bar and 0 0C is 22,710 980(38) L/mol; each mol contain 6,022 140 857.10e23 molecules.
What volume in milliliters will 0.00919 g H2 gas occupy at STP?
At STP (standard temperature and pressure: 0°C and 1 atm pressure), 1 mole of any gas occupies 22.4 liters. The molar mass of hydrogen gas (H2) is 2 g/mol. With 0.00919 g of H2, you have 0.004595 moles. So, at STP, it would occupy approximately 0.1029 liters, which is the same as 102.9 milliliters.
How many molecules (not moles) of NH3 are produced from 5.95104 g of H2?
To find the number of molecules produced, first calculate the number of moles of H2 using its molar mass. Then, use the balanced chemical equation to relate the number of moles of H2 to NH3. Finally, convert the moles of NH3 to molecules using Avogadro's number, which is 6.022 x 10^23 molecules/mol.
