HOW MANY GRAMS OF NH3 CAN BE PRODUCED FROM 15.0 G H2
H2 : NH3
= 2*1.008 : 14.007+3*1.008
= 2.016 : 17.031
So if H2 weighs 15 g, let x=NH3 produced,
cross multiply to get
mass of NH3 = 15*17.031/2.016=?
126.72
To determine the number of grams of NH3 that can be produced from 15.0 g of H2, you need to consider the balanced chemical equation for the reaction of H2 and NH3.
The balanced equation for the reaction is:
3H2 + N2 → 2NH3
From the equation, we can see that 3 moles of H2 react to produce 2 moles of NH3.
To calculate the number of moles of H2 present in 15.0 g, we need to know the molar mass of H2. Hydrogen's molar mass is approximately 2.02 g/mol.
Using the formula:
Number of moles = Mass / Molar mass
Number of moles of H2 = 15.0 g / 2.02 g/mol = 7.43 mol (approximately)
Now, we can use the stoichiometry of the reaction to determine the number of moles of NH3 produced.
From the balanced equation, we know that 3 moles of H2 react to produce 2 moles of NH3.
So, using the ratio of moles, we have:
7.43 mol H2 × (2 mol NH3 / 3 mol H2) = 4.95 mol NH3
Finally, we can calculate the mass of NH3 produced using its molar mass, which is approximately 17.03 g/mol.
Mass of NH3 = Number of moles × Molar mass
Mass of NH3 = 4.95 mol × 17.03 g/mol = 84.73 g
Therefore, approximately 84.73 grams of NH3 can be produced from 15.0 grams of H2.