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What is percent composition of AgNO2?
That depends. In a solution used for silver staining in biochemical research, for example, silver nitrate is at 0.8%, sodium hydroxide at 1.9% and ammonium hydroxide at 1.4%, with the rest made up of sterile deionized water.
How many moles of N are in 0.245g N2O?
[ 217(g) / 44.013(g/mol) ] * 2(molN/molN2O) = 9.86 mol NDivide mass (g) by molar mass (g/mol) to get moles of N2O, this should be multiplied by 2 for the stoechiometric factor of atoms N per molecule N2O.
What is the mass percentage of N in NH3?
Nitrogen has an average atomic mass of about 14 while hydrogen has an average atomic mass of about 1, so the total molecular mass of NH3 is about 17. From this we find that the mass percentage of N in NH3 is about 14/17 = 82%. To get more precise numbers, look up the exact atomic masses from a periodic table.
How many moles in a teaspoon of chalk?
The molecular weight(M) of chalk(CaCO3) = (40+12+48)g/mol =100g/mol and teaspoon (m)= 4.93g We know, n=m/M So, n= (4.93/100) mol = .0493 mol To find out number of molecules we use, N= n x NA equation. N= .0493 mol x 6.02 x 1023 molecules/mol =2.968 x 1022 molecules Therefore, there are 2.968 x 1022 molecules in a teaspoon of chalk.
How many grams of zinc contain 6x10 to the powe of 23 atoms?
To calculate the grams of zinc containing 6x10^23 atoms, we need to determine the molar mass of zinc, which is approximately 65.38 g/mol. Then, we can use Avogadro's number to find the number of moles (n) of zinc atoms: n = (6x10^23 atoms) / (6.022x10^23 atoms/mol). Finally, we can calculate the mass of zinc: mass = n x molar mass.
What is the mass of 0.0250 mol of P2O5?
3.55g
Calculate the maximum mass of ammonia that could be made from 1000g of nitrogen?
The molar mass of N is 14 g/mol and NH₃ is 17 g/mol. To find the maximum mass of NH₃ from 1000g of N, first convert 1000g N to moles (1000g / 14 g/mol = 71.43 mol). Then, use the molar ratio of N to NH₃ (1:1) to determine the maximum mass of NH₃ that can be produced (71.43 mol * 17 g/mol = 1214.71g).
What is the mass of NaNO3?
1 mol Na X (22.99 Na / mol Na) = 22.99 g Na1 mol N X (14.01 g N / mol N) = 14.01 g N3 mol O X (16.00 g O / mol O) = 48.00 g OMolar mass of NaNO3 = 85.00 g/mol
What is the molecular mass of NH3 when The atomic mass of N is 1401 gmole and the atomic mass of H is 1008 gmole?
Molecular mass = sum of all atoms masses = 1(molN/mol NH3)*14.01(g/mol N) + 3(molH/mol NH3)*1.008(g/mol H) = 17.03 g/mol NH3
How many grams are in 8.2 times 10exponets22 molecules of N2i6?
To find the mass in grams of 8.2 × 10²² molecules of N₂i₆, we first need to determine the molar mass of N₂i₆. Assuming N₂i₆ refers to a compound of nitrogen (N) and iodine (I), we would calculate its molar mass based on the atomic weights of nitrogen (approximately 14 g/mol) and iodine (approximately 127 g/mol). Once we have the molar mass, we can convert the number of molecules to moles using Avogadro's number (6.022 × 10²³ molecules/mol) and then multiply by the molar mass to find the mass in grams. Without the exact formula or molar mass, the exact mass cannot be calculated here.
What is the percentage of nitrogen in Ethylenediaminetetetraacetic acid?
Ethylenediaminetetraacetic acid (EDTA) has a chemical formula of C10H16N2O8, which contains two nitrogen (N) atoms. To calculate the percentage of nitrogen in EDTA, first determine the molar mass: C (10 × 12.01 g/mol) + H (16 × 1.008 g/mol) + N (2 × 14.01 g/mol) + O (8 × 16.00 g/mol) totals approximately 292.24 g/mol. The mass contribution from nitrogen is about 28.02 g/mol (2 × 14.01 g/mol), leading to a nitrogen percentage of approximately 9.58%.
What is the mass percent of n in ammonium bicarbonate?
The formula for ammonium bicarbonate is NH4HCO3. To find the mass percent of nitrogen (N), calculate the molar mass of nitrogen in the formula and divide it by the molar mass of the entire compound NH4HCO3. The molar mass of N is 14.01 g/mol, and the molar mass of NH4HCO3 is 79.06 g/mol. Therefore, the mass percent of nitrogen in ammonium bicarbonate is (14.01 g/mol / 79.06 g/mol) * 100% = 17.7%.
How many grams of N are in 40.8 g of N2O?
To find the grams of nitrogen (N) in 40.8 g of N₂O, first calculate the molar mass of N₂O. The molar mass is approximately 44.01 g/mol (with nitrogen being about 14.01 g/mol and oxygen about 16.00 g/mol). Since there are two nitrogen atoms in N₂O, the mass contribution from nitrogen is 28.02 g/mol. The fraction of nitrogen in N₂O is 28.02 g/mol / 44.01 g/mol = 0.636. Therefore, in 40.8 g of N₂O, there are about 25.9 g of nitrogen (40.8 g × 0.636).
What is percent composition of AgNO2?
That depends. In a solution used for silver staining in biochemical research, for example, silver nitrate is at 0.8%, sodium hydroxide at 1.9% and ammonium hydroxide at 1.4%, with the rest made up of sterile deionized water.
How many moles of N are in 0.245g N2O?
[ 217(g) / 44.013(g/mol) ] * 2(molN/molN2O) = 9.86 mol NDivide mass (g) by molar mass (g/mol) to get moles of N2O, this should be multiplied by 2 for the stoechiometric factor of atoms N per molecule N2O.
How many moles are in 2.002g of hydrogen?
To find the mole of a chemical from the given mass, use the formula mass = moles x molar mass or m = nM so to find the n... isolate the n first in the formula. n = m/M. The M signfies the Molar Mass of Hydrogen which is 1.008 g/mol and the m signifies the given mass of hydrogen which is 2.002 g. Divide 2.002 g by 1.008 g/mol which is 1.986 mol of H. Remember ... look at the units. In the formula, if you isolate M... M = m/n Since the unit of mass is g and the unit of mole is mol then m/n is the equivalent of g/mol which coincidentally is the unit of Molar mass.
What is the mass in grams of 9.15 1024 molecules of methanol CH3OH?
To find the mass of 9.15 × 10²⁴ molecules of methanol (CH₃OH), we first need to determine the molar mass of methanol, which is approximately 32.04 g/mol. Using Avogadro's number (6.022 × 10²³ molecules/mol), we can convert the number of molecules to moles: ( n = \frac{9.15 \times 10^{24}}{6.022 \times 10^{23}} \approx 15.19 ) moles. Finally, we calculate the mass: ( \text{mass} = n \times \text{molar mass} = 15.19 , \text{mol} \times 32.04 , \text{g/mol} \approx 486.4 , \text{g} ).
