the question is directing a discussion of Avagadro's number.
If Nitrogen were an ideal gas ( it isn't) there would be 6,02 X 10 ^23 atoms
One mole of atoms of an element is equal to the atomic mass of that element expressed in grams. Nitrogen-14 so one mole of nitrogen weighs 14 g
As a rule of thumb, the atomic mass of an element equals the number of grams of that element equals a mole. Since the atomic mass of Nitrogen is 14, there are 14 grams in one mole of Nitrogen. Next, we just have to divide 42 by 14 and we get our answer: There are 2.9988 moles in 42 grams of Nitrogen.
6.02 x 1023 atoms of nitrogen will weigh 14 g.So, 5.49 x 1025 atoms of nitrogen will weigh 1277 g.
The ammonium ion has one nitrogen atom and four hydrogen atoms. Their atomic masses are 14 and 1 respectively. Therefore the RMM of the ammonium ion s 14+4x1=18.
1 ounce = about 28.35 grams Therefore, 14 ounces = about 396.9 grams
One mole of atoms of an element is equal to the atomic mass of that element expressed in grams. Nitrogen-14 so one mole of nitrogen weighs 14 g
To calculate the number of atoms in 6980 grams of nitrogen, you would first convert the mass of nitrogen to moles using the molar mass of nitrogen (~14 g/mol). Then, you would use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. Overall, the calculation would be 6980 grams of nitrogen * (1 mol / 14 grams) * (6.022 x 10^23 atoms / 1 mol).
To convert grams to atoms, you need to first convert grams of nitrogen to moles using its molar mass (14.01 g/mol). Then, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. So, for 2.2 grams of nitrogen: Convert grams to moles: 2.2 g / 14.01 g/mol = 0.157 moles. Convert moles to atoms: 0.157 moles x 6.022 x 10^23 atoms/mol = 9.46 x 10^22 atoms of nitrogen.
There are 29/14, or just over 2 moles of nitrogen in 19 grams.
As a rule of thumb, the atomic mass of an element equals the number of grams of that element equals a mole. Since the atomic mass of Nitrogen is 14, there are 14 grams in one mole of Nitrogen. Next, we just have to divide 42 by 14 and we get our answer: There are 2.9988 moles in 42 grams of Nitrogen.
It is 14 - 3 = 11 grams more massive.
Nitrogen atoms, of course. Naturally occurring nitrogen has two isotopes: nitrogen-14 and nitrogen-15.
Let's see. 7.00 grams nitrogen (1 mole N/14.01 grams)(6.022 X 10^23/1 mole N) = 3.01 X 10^23 atoms of nitrogen 3.01 X 10^23 ( 1mole H/6.022 X 10^23)(1.008 grams/1 mole H) = 0.504 grams of hydrogen
6.02 x 1023 atoms of nitrogen will weigh 14 g.So, 5.49 x 1025 atoms of nitrogen will weigh 1277 g.
You would need to use 14 nitrogen-14 atoms on the right pan to balance the three calcium-42 atoms on the left pan. This is because nitrogen-14 has an atomic mass of 14, while calcium-42 has an atomic mass of 42. By multiplying the atomic mass of nitrogen-14 by 3, you would obtain a total mass of 42, thus balancing the equation.
To find the mass of nitrogen needed to make ammonia, first determine the molar mass of ammonia (NH3) which is 17 g/mol. Since there is one nitrogen atom in ammonia, the nitrogen mass is 14 g/mol. To make 34 grams of ammonia, you would need 14 grams of nitrogen.
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.