9.982 is the answer because you take the given mole and multiply it by the mass of N. So it would be 0.713 mol x 14.00 = 9.982 g
4.27562e22
5.418E23 molecules
There are 6.02 x 1023 NH3 molecules in 1 mole of NH3.Therefore 0.850mol of ammonia would have 0.85 x 6.02 x 1023 molecules of NH3.In each NH3 molecule there are 4 atoms (one N and three H atoms).Therefore the number of atoms in 0.850mol of NH3 is4 x 0.85 x 6.02 x 1023 = 2.05 x 1024
18 mol of NH3 (ammonia) contains 18 mol of N atoms. 1 mole of N2 (nitrogen gas) contains 2 mol N atoms. so 9 mol N2 is used to produce 18 mol NH3.
1 mol of any substance contains 6.02 x 1023 constituent particles. This is the avogadro constant. So in 10 moles of NH3, there would be 10 x 6.02 x 1023 = 6.02 x 1024 NH3 molecules.
There are 6.022 x 10^23 molecules in 1.00 mol of H2O2. This number is also known as Avogadro's number.
There are 3.92 x 10^22 molecules of NH3 in 0.0650 moles because one mole of NH3 contains Avogadro's number of molecules, which is 6.022 x 10^23.
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.
5.418E23 molecules
I actually have this problem in my chemistry book too. This is what is given in the "Solutions to Red Exercises" book that went along with the text: Analyze. Given: mol NH3, Find: N atoms Plan. mol NH3---> mol N atoms---> N atoms Solve. 0.410 mol NH3 * 1 mol N atoms/ 1 mol NH3 * 6.022*10^23 atoms/1mol = 2.47*10^23 N atoms Check. (0.4)(6*10^23)=2.4*10^23. I hope this helps.
To determine the grams of NH3 produced from 2.08 grams of N2, you need to set up a balanced chemical equation for the reaction. Assuming the balanced equation is N2 + 3H2 -> 2NH3, you would calculate the moles of N2, then use stoichiometry to find the moles of NH3 produced. Finally, convert moles of NH3 to grams using the molar mass of NH3.
The balanced chemical equation for the reaction between H2 and NH3 is: 3H2 + N2 → 2NH3 From the equation, we can see that 3 moles of H2 produce 2 moles of NH3. Therefore, when 1.2 moles of H2 react, we can calculate the moles of NH3 produced as: 1.2 mol H2 * (2 mol NH3 / 3 mol H2) = 0.8 mol NH3.
There are 6.02 x 1023 NH3 molecules in 1 mole of NH3.Therefore 0.850mol of ammonia would have 0.85 x 6.02 x 1023 molecules of NH3.In each NH3 molecule there are 4 atoms (one N and three H atoms).Therefore the number of atoms in 0.850mol of NH3 is4 x 0.85 x 6.02 x 1023 = 2.05 x 1024
To determine the grams of nitrogen needed, calculate the molar mass of ammonia (NH3) which is 17 grams/mole. Then, use the mole ratio from the balanced equation (1 mol N2:2 mol NH3) to find the mass of nitrogen required which is 16.5 grams.
Assuming that this ammonia gas is at STP, you can use Avogadro's number to gind the number of moles of gas:(387 x 1021 molecules) x (1 mol / 6.02x1023particles) x (17.03 g / 1 mol) =110 g NH3
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
molar mass NH3 = 17 g/molmolar mass SF6 = 146 g/molmolecules in 0.55g SF6 = 0.55g x 1mol/146g x 6.02x10^23 molecules/mole = 2.27x10^21 moleculesgrams NH3 needed = 2.27x10^21 molecules x 1mol/6.02x10^23 molecules x 17g/mol = 0.064 grams
18 mol of NH3 (ammonia) contains 18 mol of N atoms. 1 mole of N2 (nitrogen gas) contains 2 mol N atoms. so 9 mol N2 is used to produce 18 mol NH3.