Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction:
N2 (g) + 3H2(g) →2NH3 (g)
• Part A
If you have 3.32 g of H2, how many grams of NH3 can be produced?
Express your answer with the appropriate units.
To determine the amount of NH3 produced, we need to use stoichiometry and the molar ratios given in the balanced equation.
First, we need to convert the given mass of H2 to moles. The molar mass of H2 is 2.02 g/mol.
Moles of H2 = 3.32 g H2 / 2.02 g/mol H2 = 1.646 moles H2
Next, we can use the stoichiometry of the balanced equation to determine the moles of NH3 produced. According to the balanced equation, 3 moles of H2 react to produce 2 moles of NH3.
Moles of NH3 = 1.646 moles H2 × (2 moles NH3 / 3 moles H2) = 1.097 moles NH3
Finally, we can convert the moles of NH3 to grams using the molar mass of NH3, which is 17.03 g/mol.
Grams of NH3 = 1.097 moles NH3 × 17.03 g/mol NH3 = 18.68 g NH3
Therefore, 3.32 g of H2 can produce 18.68 g of NH3.
To find the mass of NH3 produced, we can use the stoichiometry of the reaction.
From the balanced equation, for every 3 moles of H2, we produce 2 moles of NH3.
First, we need to convert the given mass of H2 to moles.
The molar mass of H2 is 2 g/mol (2 hydrogen atoms x 1 g/mol).
Using the molar mass, we can calculate the number of moles:
Number of moles of H2 = mass of H2 / molar mass of H2
= 3.32 g / 2 g/mol
= 1.66 mol
Now, we can use the mole ratio from the balanced equation to determine the moles of NH3 produced.
According to the balanced equation, 3 moles of H2 will produce 2 moles of NH3.
Therefore, the moles of NH3 produced can be calculated as:
Number of moles of NH3 = (2 moles of NH3 / 3 moles of H2) x (1.66 mol of H2)
= 1.10 mol
Finally, we need to convert the moles of NH3 to grams.
The molar mass of NH3 is 17 g/mol (14 g/mol for nitrogen + 3 g/mol for each hydrogen atom).
Using the molar mass, we can calculate the mass of NH3:
Mass of NH3 = number of moles of NH3 x molar mass of NH3
= 1.10 mol x 17 g/mol
= 18.7 g
Therefore, 3.32 g of H2 can produce 18.7 g of NH3.
To determine the grams of NH3 that can be produced when 3.32 g of H2 is reacted, we need to use the stoichiometry of the reaction.
First, we need to calculate the moles of H2 by dividing the given mass by its molar mass. The molar mass of H2 is 2 g/mol, so:
Moles of H2 = mass of H2 / molar mass of H2
= 3.32 g / 2 g/mol
= 1.66 mol
According to the balanced equation, the stoichiometric ratio between H2 and NH3 is 3:2. This means that for every 3 moles of H2, 2 moles of NH3 are produced.
Now, we can calculate the moles of NH3 produced using the stoichiometry:
Moles of NH3 = (Moles of H2) * (2 moles NH3 / 3 moles H2)
= 1.66 mol * (2/3)
= 1.1067 mol
Finally, to find the mass of NH3 produced, we use the moles of NH3 and its molar mass. The molar mass of NH3 is 17 g/mol:
Mass of NH3 = moles of NH3 * molar mass of NH3
= 1.1067 mol * 17 g/mol
= 18.81 g
Therefore, when 3.32 g of H2 reacts, approximately 18.81 g of NH3 can be produced.