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To determine the number of moles of N2O3 containing 2.55 x 10^24 oxygen atoms, we first calculate the molar mass of N2O3, which is 76.01 g/mol. Next, we find the number of moles of oxygen atoms in 2.55 x 10^24 atoms by dividing the given number by Avogadro's number (6.022 x 10^23 atoms/mol). This gives us approximately 4.24 moles of oxygen atoms. Since each mole of N2O3 contains 3 moles of oxygen atoms, the number of moles of N2O3 containing 2.55 x 10^24 oxygen atoms is 4.24 moles / 3 = 1.41 moles.
To find the number of moles of N2O3 containing 2.55 x 10^24 oxygen atoms, we first determine the number of moles in 2.55 x 10^24 oxygen atoms by dividing by Avogadro's number (6.022 x 10^23). This gives us the number of moles of O atoms. Since one mole of N2O3 contains 3 moles of oxygen atoms, we can then convert moles of O atoms to moles of N2O3 by dividing by 3.
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What is the total number of moles of oxygen atoms in 1 mole of N2O3?
There are 3 oxygen atoms in 1 molecule of N2O3. Since there is only 1 mole of N2O3, there are 3 moles of oxygen atoms in total.
How many molecules are in 75g of N2O3?
To find the number of molecules in 75g of N2O3, you first need to calculate the number of moles using the molecular weight of N2O3 (76.01 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
What is the best name for a compound made from nitrogen and oxygen (N2O3)?
The best name for a compound made from nitrogen and oxygen (N2O3) is nitrogen trioxide.
Is n2o3 ionic or covalent compound?
N2O3 is a covalently bonded compound, since neither nitrogen nor oxygen is a metal or semi-metal.
Is N2O3 a ionic or covalent compound?
N2O3 is a covalent compound. It consists of nonmetal elements (nitrogen and oxygen) that share electrons through covalent bonds to form molecules.
What is the total number of moles of oxygen atoms in 1 mole of N2O3?
There are 3 oxygen atoms in 1 molecule of N2O3. Since there is only 1 mole of N2O3, there are 3 moles of oxygen atoms in total.
How many molecules are in 75g of N2O3?
To find the number of molecules in 75g of N2O3, you first need to calculate the number of moles using the molecular weight of N2O3 (76.01 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
What is the best name for a compound made from nitrogen and oxygen (N2O3)?
The best name for a compound made from nitrogen and oxygen (N2O3) is nitrogen trioxide.
Is n2o3 ionic or covalent compound?
N2O3 is a covalently bonded compound, since neither nitrogen nor oxygen is a metal or semi-metal.
Is N2O3 a ionic or covalent compound?
N2O3 is a covalent compound. It consists of nonmetal elements (nitrogen and oxygen) that share electrons through covalent bonds to form molecules.
What is Dinitrogen trioxides formula?
The formula for dinitrogen trioxide is N2O3. It is a chemical compound composed of two nitrogen atoms and three oxygen atoms.
What is the chemical formula for 2 nitrogen and 3 oxygen?
The dinitrogen trioxide is N2O3.
What is the Formula for dintrogen trioxide?
The chemical formula for dinitrogen trioxide is N2O3, consisting of two nitrogen atoms and three oxygen atoms.
What is the oxidation number of n2o3?
In N2O3, the oxidation state of nitrogen is +3 because oxygen is usually assigned an oxidation state of -2, and there are three oxygen atoms in N2O3. The sum of the oxidation states in a neutral compound should be zero, so the oxidation state of nitrogen must be +3 in order to balance the -6 from the three oxygen atoms.
Is N2O3 a covalent and an ionic bond?
N2O3 consists of covalent bonds. It is a molecule formed by the sharing of electrons between nitrogen and oxygen atoms. Ionic bonds involve the transfer of electrons between a metal and a non-metal, which is not the case in N2O3.
Is N2O3 ionic or molecular?
molecular
What is the ratio of nitrogen atoms to oxygen atoms in dinitrogen trioxide?
The ratio of nitrogen atoms to oxygen atoms in dinitrogen trioxide (N2O3) is 2:3. This is because the compound contains 2 nitrogen atoms and 3 oxygen atoms.
