4NH3 + 5O2 ---> 4NO + 6H2O
The moles of NH3= the moles of NO
15 moles of NO*(30.01g of NO/mol)= g of NO
The moles of NH3= the moles of NO
15 moles of NO*(30.01g of NO/mol)= g of NO
The balanced chemical equation for the reaction between NH3 and NO is as follows:
4 NH3 + 6 NO -> 5 N2 + 6 H2O
From the equation, we can see that for every 4 moles of NH3, 5 moles of N2 are produced.
Step 1: Calculate the moles of N2 produced using the mole ratio:
Moles of N2 = (15.0 moles of NH3) x (5 moles of N2 / 4 moles of NH3)
Moles of N2 = 18.75 moles of N2
Step 2: Convert moles of N2 to grams using the molar mass:
Molar mass of N2 = 28.02 g/mol
Mass of N2 = (18.75 moles of N2) x (28.02 g/mol)
Mass of N2 = 524.57 grams of N2
Therefore, when 15.0 moles of NH3 react with excess NO, 524.57 grams of N2 are produced.
4 NH3 + 6 NO --> 5 N2 + 6 H2O
From the balanced equation, we can see that 4 moles of NH3 react with 6 moles of NO to produce 5 moles of N2.
To find the number of moles of N2 produced, we can use the given information about NH3:
15.0 moles of NH3
Using the mole ratio from the balanced equation, we can set up the following conversion:
15.0 moles NH3 x (5 moles N2 / 4 moles NH3) = moles of N2
Now, we can calculate the moles of N2 produced:
15.0 moles NH3 x (5 moles N2 / 4 moles NH3) = 18.75 moles N2
Finally, we need to convert the moles of N2 into grams. To do this, we need to use the molar mass of N2, which is approximately 28.02 g/mol.
To convert moles to grams, we multiply by the molar mass:
18.75 moles N2 x 28.02 g/mol = 524.625 grams N2
Therefore, approximately 524.63 grams of N2 are produced when 15.0 moles of NH3 react with excess NO.