Rank the following fertilizers in decreasing order of mass percentage of nitrogen:
NH3
NH4NO3
(NH4)2HPO4
KNO3
(NH4)H2PO4
(NH4)2SO4
NH3
NH4NO3
(NH4)2HPO4
(NH4)2SO4
KNO3
(NH4)H2PO4
NH3
NH4NO3
(NH4)2HPO4
(NH4)2SO4
KNO3
(NH4)H2PO4
You need to work out the mass percentage of N in each. So in each case you need to the molar mass then calculate the % N content from
Total mass of N x100%/(molar mass)
Sure, let's have some fun with this!
Okay, so let's start from the highest mass percentage of nitrogen and move our way down:
1. NH3 (Ammonia) - Well, it's got "N" "H" "3" in it, so we can safely assume it's 100% nitrogen! Just kidding. It is actually only about 82% nitrogen by mass. Still pretty impressive though!
2. NH4NO3 (Ammonium nitrate) - This one is a bit less funny. It contains about 35% nitrogen by mass.
3. KNO3 (Potassium nitrate) - Ah, potassium nitrate! Sure, it's got potassium, but we're here for nitrogen! It contains about 14% nitrogen by mass. It's not at the top of the nitrogen game, but it's still better than just pure potassium!
4. (NH4)2SO4 (Ammonium sulfate) - Ah, the sulfate gang! This one contains around 21% nitrogen by mass. Not too shabby!
5. (NH4)2HPO4 (Ammonium phosphate) - This one is a bit lower on the nitrogen side, with about 16% nitrogen by mass. It's not rocking the nitrogen world, but it's doing its thing.
6. (NH4)H2PO4 (Monoammonium phosphate) - And last, but certainly not least, this fertilizer contains around 11% nitrogen by mass. It's not as high in nitrogen content as the others, but it's still an important player in the fertilizer game.
So, there you have it, in decreasing order of mass percentage of nitrogen: NH3, NH4NO3, (NH4)2SO4, (NH4)2HPO4, KNO3, and (NH4)H2PO4. Hope this answer tickled your fertilizer funny bone!
To rank the fertilizers in decreasing order of mass percentage of nitrogen, we first need to determine how much nitrogen is present in each fertilizer compound.
1. NH3 (Ammonia) - Ammonia (NH3) is a gas and does not contain any nitrogen in a solid state. Therefore, we can exclude it from our ranking.
2. NH4NO3 (Ammonium Nitrate) - Ammonium nitrate (NH4NO3) consists of ammonium ions (NH4+) and nitrate ions (NO3-). To calculate the mass percentage of nitrogen, divide the molar mass of nitrogen by the molar mass of ammonium nitrate, and multiply by 100:
(Nitrogen molar mass / Ammonium nitrate molar mass) * 100
Nitrogen's molar mass = 14.01 g/mol
Ammonium nitrate's molar mass = 80.04 g/mol + 14.01 g/mol + (3 * 16.00 g/mol)
Calculate the percentage of nitrogen for NH4NO3.
(14.01 g/mol / 80.04 g/mol + 14.01 g/mol + (3 * 16.00 g/mol)) * 100 = 35.0%
Thus, NH4NO3 has a mass percentage of nitrogen of 35.0%.
3. (NH4)2HPO4 (Diammonium phosphate) - Diammonium phosphate ((NH4)2HPO4) contains two ammonium ions (NH4+) and one phosphate ion (HPO42-). We will follow the same process as above to calculate the mass percentage of nitrogen:
(2 * Nitrogen molar mass / Diammonium phosphate molar mass) * 100
Calculate the percentage of nitrogen for (NH4)2HPO4.
(2 * 14.01 g/mol / (2 * 14.01 g/mol) + 63.99 g/mol + 2 * (1.01 g/mol + 32.00 g/mol)) * 100 = 18.8%
Thus, (NH4)2HPO4 has a mass percentage of nitrogen of 18.8%.
4. KNO3 (Potassium nitrate) - Potassium nitrate (KNO3) consists of potassium ions (K+) and nitrate ions (NO3-). The process for calculating the mass percentage of nitrogen remains the same:
(Nitrogen molar mass / Potassium nitrate molar mass) * 100
Calculate the percentage of nitrogen for KNO3.
(14.01 g/mol / 101.10 g/mol + 14.01 g/mol + (3 * 16.00 g/mol)) * 100 = 13.7 %
Thus, KNO3 has a mass percentage of nitrogen of 13.7%.
5. (NH4)H2PO4 (Monoammonium phosphate) - Monoammonium phosphate ((NH4)H2PO4) contains one ammonium ion (NH4+) and one phosphate ion (H2PO4-). To calculate the mass percentage of nitrogen:
(Nitrogen molar mass / Monoammonium phosphate molar mass) * 100
Calculate the percentage of nitrogen for (NH4)H2PO4.
(14.01 g/mol / 14.01 g/mol + 3 * (1.01 g/mol) + 2 * (1.01 g/mol + 32.00 g/mol)) * 100 = 12.6%
Thus, (NH4)H2PO4 has a mass percentage of nitrogen of 12.6%.
6. (NH4)2SO4 (Ammonium sulfate) - Ammonium sulfate ((NH4)2SO4) consists of two ammonium ions (NH4+) and one sulfate ion (SO42-). As before, we'll use the same method to calculate the mass percentage of nitrogen:
(2 * Nitrogen molar mass / Ammonium sulfate molar mass) * 100
Calculate the percentage of nitrogen for (NH4)2SO4.
(2 * 14.01 g/mol / (2 * 14.01 g/mol) + 2 * (1.01 g/mol) + 4 * 16.00 g/mol) * 100 = 21.2%
Thus, (NH4)2SO4 has a mass percentage of nitrogen of 21.2%.
Ranking the fertilizers in decreasing order of mass percentage of nitrogen:
1. NH4NO3 (Ammonium Nitrate) - 35.0%
2. (NH4)2SO4 (Ammonium Sulfate) - 21.2%
3. (NH4)2HPO4 (Diammonium Phosphate) - 18.8%
4. (NH4)H2PO4 (Monoammonium Phosphate) - 12.6%
5. KNO3 (Potassium Nitrate) - 13.7%
i worked out the mass percentage of N in each and this is what i got
NH3=82.25%
NH4NO3=35%
(NH4)2HPO4=21.4%
KNO3=13.85%
(NH4)H2PO4=12.17%
(NH4)2SO4=11.85%
i put in order and still get it wrong -__-
Total mass of N x100%/(molar mass)