How many grams of H2 are needed to produce 11.61 grams of NH3?
a mole of NH3 is composed of one mole of N and three moles of H
find the molar mass of NH3
... find the moles in 11.61 g ... 11.61 g / molar mass
find the moles of H ... three times moles of NH3
find the grams of H ... moles * molar mass
To determine the number of grams of H2 needed to produce a certain amount of NH3, you can use stoichiometry.
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 are needed to produce 2 moles of NH3.
To solve the problem, we need to follow these steps:
1. Calculate the molar mass of NH3:
The molar mass of NH3 is calculated by adding the atomic masses of its constituent atoms. Nitrogen (N) has a molar mass of 14.01 g/mol, and hydrogen (H) has a molar mass of 1.01 g/mol (since there are three hydrogen atoms in NH3). Adding them up, we get:
Molar mass of NH3 = 14.01 g/mol + (1.01 g/mol x 3) = 17.04 g/mol.
2. Since the molar mass of NH3 is 17.04 g/mol, we can calculate the number of moles of NH3 using the formula:
Moles of NH3 = Mass of NH3 / Molar mass of NH3.
Moles of NH3 = 11.61 g NH3 / 17.04 g/mol = 0.682 moles NH3.
3. Now, using the stoichiometric ratio from the balanced equation, we can determine the moles of H2 required to react with the given moles of NH3.
For every 2 moles of NH3, we need 3 moles of H2.
Moles of H2 = (3 moles H2 / 2 moles NH3) x 0.682 moles NH3 = 1.023 moles H2.
4. Finally, we need to calculate the mass of H2 in grams using its molar mass:
Molar mass of H2 = 2.02 g/mol.
Mass of H2 = Moles of H2 x Molar mass of H2.
Mass of H2 = 1.023 moles H2 x 2.02 g/mol = 2.07 grams of H2.
Therefore, to produce 11.61 grams of NH3, approximately 2.07 grams of H2 are needed.