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A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. Determine molecular formula and the accurate molar mass.?
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. The molecular formula and the accurate molar mass would be N14O35.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen and 8 grams of oxygen form how many grams of water form?
the same amount would have to stay in grams, so if 14 grams of nitrogen is formed, then 8 grams of oxygen, add those two together and you get 22. and that's 22 of the 40 grams used, so 40 subtracted by 22 is 18. 18 grams of water would be formed.
The formula for nitrogen dioxide is NO2 What is the molar mass of nitrogen dioxide to the nearest gram?
The molar mass of nitrogen (N) is approximately 14 grams/mole, and the molar mass of oxygen (O) is approximately 16 grams/mole. Therefore, the molar mass of nitrogen dioxide (NO2) is 14 + (2*16) = 46 grams/mole to the nearest gram.
If a compound is 26 percent nitrogen and 74 percent oxygen what is the emprical formula?
First you want to think "if I had 100 grams of this compound". If you do this, then you will be able to use the percentages as measurements in grams. Completing the sentence: "if I had 100 grams of this compound, then I would have 26 grams of nitrogen and 74 grams of oxygen". The next step is converting the grams to moles.Grams ÷ Atomic weight = moles26.0 grams ÷ 14.0 grams = 1.86 moles N74.0 grams ÷ 16.0 grams = 4.63 moles OThis is a ratio of 1.86:4.63 and is not recognizable as a small whole number ratio. (If this doesn't make sense, see the Law of Definite Proportions). In order to make the two numbers whole numbers, a trick is to divide both by the smallest number. Doing this will ensure that one number will always be 1.1.86 moles N ÷ 1.86 = 14.63 moles O ÷ 1.86 = 2.49Because the last digit is always uncertain to .02, we can say that 2.49 is actually 2.5. Now your ratio is 1:2.5, yet these are still not whole numbers. When you have an increment of .5, then multiply everything by 2.1:2.5 × 2 = 2:5 or 2 nitrogen : 5 oxygenYour final answer is N2O5
What is N4Se4?
N4Se4 is a chemical compound consisting of nitrogen and selenium atoms in a specific combination. It is a molecular compound with a tetrahedral structure and is known for its interesting electronic properties.
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. Determine molecular formula and the accurate molar mass.?
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. The molecular formula and the accurate molar mass would be N14O35.
A compound is formed when 48 grams of carbon 8 grams of hydrogen and 68 grams oxygen combine what is the percent by mass of oxygen?
The percentage of oxygen is 54,84 %.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen and 8 grams of oxygen form how many grams of water form?
the same amount would have to stay in grams, so if 14 grams of nitrogen is formed, then 8 grams of oxygen, add those two together and you get 22. and that's 22 of the 40 grams used, so 40 subtracted by 22 is 18. 18 grams of water would be formed.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen qnd 8 grams of oxygen form How many grams of water form?
if 14 grams of nitrogen is formed, then 8 grams of oxygen, add those two together and you get 22. and that's 22 of the 40 grams used, so 40 subtracted by 22 is 18. 18 grams of water would be formed.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen and 8 grams of oxygen form.. How many grams of water form?
the same amount would have to stay in grams, so if 14 grams of nitrogen is formed, then 8 grams of oxygen, add those two together and you get 22. and that's 22 of the 40 grams used, so 40 subtracted by 22 is 18. 18 grams of water would be formed.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen and 8 grams of oxygen form. How many grams of water form?
the same amount would have to stay in grams, so if 14 grams of nitrogen is formed, then 8 grams of oxygen, add those two together and you get 22. and that's 22 of the 40 grams used, so 40 subtracted by 22 is 18. 18 grams of water would be formed.
The formula for nitrogen dioxide is NO2 What is the molar mass of nitrogen dioxide to the nearest gram?
The molar mass of nitrogen (N) is approximately 14 grams/mole, and the molar mass of oxygen (O) is approximately 16 grams/mole. Therefore, the molar mass of nitrogen dioxide (NO2) is 14 + (2*16) = 46 grams/mole to the nearest gram.
If a compound is 26 percent nitrogen and 74 percent oxygen what is the emprical formula?
First you want to think "if I had 100 grams of this compound". If you do this, then you will be able to use the percentages as measurements in grams. Completing the sentence: "if I had 100 grams of this compound, then I would have 26 grams of nitrogen and 74 grams of oxygen". The next step is converting the grams to moles.Grams ÷ Atomic weight = moles26.0 grams ÷ 14.0 grams = 1.86 moles N74.0 grams ÷ 16.0 grams = 4.63 moles OThis is a ratio of 1.86:4.63 and is not recognizable as a small whole number ratio. (If this doesn't make sense, see the Law of Definite Proportions). In order to make the two numbers whole numbers, a trick is to divide both by the smallest number. Doing this will ensure that one number will always be 1.1.86 moles N ÷ 1.86 = 14.63 moles O ÷ 1.86 = 2.49Because the last digit is always uncertain to .02, we can say that 2.49 is actually 2.5. Now your ratio is 1:2.5, yet these are still not whole numbers. When you have an increment of .5, then multiply everything by 2.1:2.5 × 2 = 2:5 or 2 nitrogen : 5 oxygenYour final answer is N2O5
How many grams of nitrogen in one gallon of pure water?
None. Pure water has only hydrogen and oxygen.
How much nitrogen is in 7.5 grams of ammonia?
First you need to find the atomic masses of each element involved in the compound NH3, and add them up to find the total molecular mass of ammonia.Nitrogen = 14.0 gramsHydrogen = 1.01 × 3 atoms = 3.03 grams----------------------------------------------------Ammonia = 17.03 gramsThen you take the mass of nitrogen in one molecule and divide it by the total mass to find the percent composition.14.0 grams Nitrogen ÷ 17.03 grams Ammonia = .822 = 82.2% nitrogen in ammoniaThen you simply need to take 82.2% of 7.5 grams to find how much nitrogen is in that particular amount.82.2% × 7.50 = 6.17 grams of nitrogen in 7.50 grams of ammonia
How many moles of nitrogen are in 15 grams of nitrogen?
15 grams of nitrogen are equal to 1,071 moles.
How many grams of potassium chlorate will produce 112.5g of oxygen?
To calculate the amount of potassium chlorate needed to produce 112.5g of oxygen, you first need to determine the molar ratio between potassium chlorate and oxygen. Then, use this ratio to convert the grams of oxygen to grams of potassium chlorate using the molar masses of each compound.
