What is the maximum mass, in grams, of NH3 that can be produced by the reaction of 1.0 g of N2 and 1.0 g of H2 using the reaction below?
N2+H2→NH3 (not balanced)
What is the maximum mass, in grams, of that can be produced by the reaction of 1.0 g of and 1.0 g of using the reaction below?
(not balanced)
A) 0.60 g
B) 5.7 g
C) 1.2 g
D) 2.9 g
See your post above.
To answer this question, we need to calculate the maximum mass of NH3 that can be produced by the given reaction. First, let's balance the chemical equation:
N2 + 3H2 → 2NH3
Now that the equation is balanced, we can use the concept of stoichiometry, which relates the amounts of reactants and products in a chemical reaction.
The balanced equation tells us that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. We can use the molar masses of N2, H2, and NH3 to convert the given masses into moles:
Molar mass of N2 = 14.01 g/mol
Molar mass of H2 = 2.02 g/mol
Molar mass of NH3 = 17.03 g/mol
For N2:
1.0 g N2 * (1 mol N2 / 14.01 g N2) = 0.071 mol N2
For H2:
1.0 g H2 * (1 mol H2 / 2.02 g H2) = 0.495 mol H2
Since the reaction ratio is 1:3 for N2 to H2, we need to compare the number of moles of N2 and H2 to determine the limiting reactant. Since we have excess H2 (0.495 mol) and only 0.071 mol of N2, N2 is the limiting reactant. This means that it will completely react, and any excess H2 will remain unreacted.
Using the molar ratio from the balanced equation, we can calculate the number of moles and then convert it to mass for NH3:
0.071 mol N2 * (2 mol NH3 / 1 mol N2) * (17.03 g NH3 / 1 mol NH3) = 2.43 g NH3
Therefore, the maximum mass of NH3 that can be produced from 1.0 g of N2 and 1.0 g of H2 is approximately 2.43 grams.
Looking at the provided answer choices, none of them match the calculated value. Please double-check the answer choices or the information given in the question.