Which of the following nitrogen-containing compounds would supply the most nitrogen per gram of fertilizer?
a. iron azide, Fe(N3)2, MW = 140 g/mol
b. sodium azide, NaN3, MW = 65 g/mol
c. potassium nitrite, KNO2, MW = 85.1 g/mol
d. potassium azide, KN3, MW = 81.1 g/mol
e. There is not enough information to answer this problem
Could you please explain how to solve this?
I would calculate the percentage of N in each of the compounds. The with the highest percentage will supply the most N per grams, per pound, per anything.
You can do it another way. Convert 1 g of the compound to ? grams of N. For example, #1 would be
1 g Fe(N3)2 x (6*atomic mass N)/molar mas Fe(N3)2 = g N
To determine which nitrogen-containing compound would supply the most nitrogen per gram of fertilizer, we need to calculate the number of moles of nitrogen in each compound and compare them. The compound with the highest number of moles of nitrogen per gram of fertilizer will supply the most nitrogen.
Let's calculate the moles of nitrogen for each compound using the given molecular weights:
a. iron azide, Fe(N3)2, MW = 140 g/mol
The molecular weight of nitrogen, N, is 14 g/mol.
Number of moles of nitrogen = 2 moles of N = 2 * 14 g/mol = 28 g/mol
b. sodium azide, NaN3, MW = 65 g/mol
Number of moles of nitrogen = 1 mole of N = 1 * 14 g/mol = 14 g/mol
c. potassium nitrite, KNO2, MW = 85.1 g/mol
Number of moles of nitrogen = 1 mole of N = 1 * 14 g/mol = 14 g/mol
d. potassium azide, KN3, MW = 81.1 g/mol
Number of moles of nitrogen = 1 mole of N = 1 * 14 g/mol = 14 g/mol
Comparing the number of moles of nitrogen for each compound, we find:
a. iron azide, Fe(N3)2: 28 g/mol
b. sodium azide, NaN3: 14 g/mol
c. potassium nitrite, KNO2: 14 g/mol
d. potassium azide, KN3: 14 g/mol
Therefore, the compound that would supply the most nitrogen per gram of fertilizer is iron azide, Fe(N3)2, with 28 g/mol of nitrogen. The correct answer is (a) iron azide.
To determine which of the given nitrogen-containing compounds supplies the most nitrogen per gram of fertilizer, we need to compare their molar masses.
The molar mass of a compound is the mass, in grams, of one mole of that compound. It is calculated by adding up the atomic masses of all the atoms in the chemical formula.
Now, we can calculate the molar mass for each compound:
a. iron azide, Fe(N3)2, MW = 140 g/mol
b. sodium azide, NaN3, MW = 65 g/mol
c. potassium nitrite, KNO2, MW = 85.1 g/mol
d. potassium azide, KN3, MW = 81.1 g/mol
To calculate the amount of nitrogen per gram of fertilizer, we divide the molar mass of nitrogen (14 g/mol) by the molar mass of the compound.
So, for each compound:
a. nitrogen per gram = 14 g/mol / 140 g/mol = 0.1 g nitrogen/gram of fertilizer
b. nitrogen per gram = 14 g/mol / 65 g/mol = 0.215 g nitrogen/gram of fertilizer
c. nitrogen per gram = 14 g/mol / 85.1 g/mol = 0.164 g nitrogen/gram of fertilizer
d. nitrogen per gram = 14 g/mol / 81.1 g/mol = 0.173 g nitrogen/gram of fertilizer
Comparing the nitrogen per gram of fertilizer value, we find that sodium azide (NaN3) supplies the most nitrogen, with 0.215 g of nitrogen per gram of fertilizer.
Therefore, the answer is (b) sodium azide, NaN3, which supplies the most nitrogen per gram of fertilizer.