Based on the following balanced equation:
2 NH3 + 2 O2 -->N2O + 3 H2O
a. How many moles of O2 are required to react completely with 6.00 moles of NH3?
b. How many grams of O2 are required to react completely with 6.00 moles of NH3?
c. How many moles of H2O are produced after complete reaction of 6.00 moles of NH3?
d. How many grams of H2O are produced after complete reaction of 6.00 moles of NH3?
These are my answers:
a. 12.0 mol O2
b. 384 g O2
c. 9.00 mol H2O
d. 162 g H2O
a is not right.
6 mols NH3 x (2 mols O2/2 mol NH3) = 6 mols O2.
b. just half that since a is 2x too high.
c and d are ok.
To find the answers to these questions, we'll use stoichiometry, which is the calculation of quantities in a chemical reaction based on balanced equations. Here's how to solve each part:
a. How many moles of O2 are required to react completely with 6.00 moles of NH3?
Looking at the balanced equation: 2 NH3 + 2 O2 → N2O + 3 H2O
We can see that 2 moles of NH3 react with 2 moles of O2. Therefore, if 2 moles of NH3 require 2 moles of O2, then 6 moles of NH3 will require (6/2) × 2 = 12 moles of O2.
So the answer is 12.0 moles of O2.
b. How many grams of O2 are required to react completely with 6.00 moles of NH3?
To find the grams of O2, we need to use the molar mass of O2, which is 32.00 g/mol.
Using the result from part (a), we have 12.0 moles of O2. To convert moles to grams, we multiply by the molar mass:
12.0 moles O2 x 32.00 g/mol = 384 g O2
So the answer is 384 g O2.
c. How many moles of H2O are produced after complete reaction of 6.00 moles of NH3?
From the balanced equation, we can see that 2 moles of NH3 produce 3 moles of H2O. Therefore, if 2 moles of NH3 produce 3 moles of H2O, then 6 moles of NH3 will produce (6/2) × 3 = 9 moles of H2O.
So the answer is 9.00 moles of H2O.
d. How many grams of H2O are produced after complete reaction of 6.00 moles of NH3?
Using the molar mass of H2O, which is 18.02 g/mol:
9.00 moles H2O x 18.02 g/mol = 162 g H2O
So the answer is 162 g H2O.
Therefore, your answers are correct.