Atomic Mass ratio for O : N is 15.9994 : 14.0067 .
So it takes 14.0067/15.9994 moles of Oxygen to have the same mass as one mole of nitrogen. This is valuated at 0.8754516 to 1.00000
Both nitrogen and oxygen exist at standard temperature and pressure as diatomic molecules. Therefore, the relative masses of equal numbers of molecules of the substance will the same as the ratios of their atomic masses, which are 15.9994 for oxygen and 14.0067 for nitrogen. The mass of oxygen that contains the same number of molecules as 42 g of nitrogen is 42(15.9994/14.0067) or 48 g, to the justified number of significant digits.
Compared to the (charge/mass) ratio of the electron:-- The (charge/mass) ratio of the proton is much smaller; although the proton charge is equal to the electron charge, the proton mass is much larger, by a factor of more than 1,800.-- The (charge/mass) ratio of the neutron is zero, because the neutron charge is zero.
No, one mole of each, having the same VOLUME (about 22.4 L at STP), differ though in their masses: 32 g/mol for O2 and 28 g/mol for N2 So their densities (mass per volume) also differ in the same way: 1.43 g/L and 1.25 g/L respectively, at STP.
You are talking about a natural isotope of nitrogen i.e Nitrogen-15 which has atomic number same as nitrogen (7) ans mass number 1 greater than standard nitrogen (i.e 15 as Nitrogen's mass no. is 14). Nitrogen-15 has i neutron more than standard nitrogen
Nitrogen-14 and nitrogen-15 are both isotopes of nitrogen, meaning they have the same number of protons but a different number of neutrons. They both belong to the same chemical element and share similar chemical properties. The main difference between them is their atomic mass, with nitrogen-15 having one extra neutron compared to nitrogen-14.
Both nitrogen and oxygen exist at standard temperature and pressure as diatomic molecules. Therefore, the relative masses of equal numbers of molecules of the substance will the same as the ratios of their atomic masses, which are 15.9994 for oxygen and 14.0067 for nitrogen. The mass of oxygen that contains the same number of molecules as 42 g of nitrogen is 42(15.9994/14.0067) or 48 g, to the justified number of significant digits.
No elements have the same average mass, but some isotopes are the same mass as other elements, For example Carbon-13 (an isotope of carbon) has the same mass as nitrogen-13 (which is also an isotope of nitrogen).
The atomic mass number of nitrogen is 14.0
The nitrogen oxides that have the same empirical formula are nitric oxide (NO) and nitrogen dioxide (NO2). Both have a 1:1 ratio of nitrogen to oxygen atoms.
The ratio is the same. Inertia depends entirely on mass.
They have the same mass/charge ratio.
The atomic weight is14.00674
Both nitrogen and oxygen exist at standard temperature and pressure as diatomic molecules. Therefore, the relative masses of equal numbers of molecules of the substance will the same as the ratios of their atomic masses, which are 15.9994 for oxygen and 14.0067 for nitrogen. The mass of oxygen that contains the same number of molecules as 42 g of nitrogen is 42(15.9994/14.0067) or 48 g, to the justified number of significant digits.
Compared to the (charge/mass) ratio of the electron:-- The (charge/mass) ratio of the proton is much smaller; although the proton charge is equal to the electron charge, the proton mass is much larger, by a factor of more than 1,800.-- The (charge/mass) ratio of the neutron is zero, because the neutron charge is zero.
These ratios are not identical. In N2O5 the ratio is 2/5. In NO2 the ratio is 1/2.
The first person to recognize the total ratio of the number atoms is the same as the total ratio of the ratio of the mass is JOHN DALTON.This is also called the "Law of Multiple Proportion"
The same 2 to 3 because the mass is directly proportional to the volume. Recall the relationship Mass = volume x density. Here density remains constant