12. Find the mass in grams, of 1.00times 10^23 molecules of N_(2) 13. How many particles are there in 1.43 g of a compound with a gram formula mass of 233 g? 14. How many grams are there in 3.4times 10^24 molecules of NH_(3) 15. Aspartame is an artificial sweetener therts 760 times speeter than sucrose (table sugar)when dissolved in water It is market to by G.D. Searle as Nutra Sweet.The molecular formula of aspartame is C_(14)H_(1)O_(2)O_(5) a) Calculate the gram formula-mass of aspartame. b) How many molecules are in 10 g of aspartame?

12. To find the mass of molecules of , we need to use Avogadro's number, which is molecules/mol. First, we need to find the molar mass of . The atomic mass of nitrogen (N) is approximately 14.01 g/mol. Since has two nitrogen atoms, its molar mass is g/mol.Now, we can calculate the mass of molecules of :Mass = (Number of molecules) x (Molar mass) / (Avogadro's number)Mass = ( molecules) x (28.02 g/mol) / ( molecules/mol)Mass ≈ 4.65 gTherefore, the mass of molecules of is approximately 4.65 grams.13. To find the number of particles in 1.43 g of a compound with a gram formula mass of 233 g, we can use the concept of moles.First, we need to calculate the number of moles in 1.43 g of the compound:Number of moles = Mass / Molar massNumber of moles = 1.43 g / 233 g/molNumber of moles ≈ 0.00612 molNow, we can calculate the number of particles using Avogadro's number:Number of particles = Number of moles x Avogadro's numberNumber of particles = 0.00612 mol x ( particles/mol)Number of particles ≈ particlesTherefore, there are approximately particles in 1.43 g of the compound.14. To find the mass of molecules of , we need to use Avogadro's number and the molar mass of .The molar mass of is calculated as follows:Molar mass of N = 14.01 g/molMolar mass of H = 1.01 g/molMolar mass of = 14.01 g/mol + (3 x 1.01 g/mol) = 17.04 g/molNow, we can calculate the mass of molecules of :Mass = (Number of molecules) x (Molar mass) / (Avogadro's number)Mass = ( molecules) x (17.04 g/mol) / ( molecules/mol)Mass ≈ 95.5 gTherefore, the mass of molecules of is approximately 95.5 grams.15. a) To calculate the gram formula-mass of aspartame ( ), we need to sum the atomic masses of all the atoms in the molecule:Atomic mass of C = 12.01 g/molAtomic mass of H = 1.01 g/molAtomic mass of N = 14.01 g/molAtomic mass of O = 16.00 g/molGram formula-mass of aspartame = (14 x 12.01) + (18 x 1.01) + (2 x 14.01) + (5 x 16.00)Gram formula-mass of aspartame = 168.14 + 18.18 + 28.02 + 80.00Gram formula-mass of aspartame = 294.34 g/molTherefore, the gram formula-mass of aspartame is 294.34 g/mol.b) To find the number of molecules in 10 g of aspartame, we can use the concept of moles.First, we need to calculate the number of moles in 10 g of aspartame:Number of moles = Mass / Molar massNumber of moles = 10 g / 294.34 g/molNumber of moles ≈ 0.034 molNow, we can calculate the number of molecules using Avogadro's number:Number of molecules = Number of moles x Avogadro's numberNumber of molecules = 0.034 mol x ($6.022\times