* Assuming it's liquid * Molecular weight : 28.0134 g/mol * Liquid density (1.013 bar at boiling point) : 808.607 kg/m3=808.607g/L 10.5L = 8490.3735 g divide by 28.0134 = 303.0825 mol
The number of atoms is 45,166.10e23.
Give the number of moles of N2 in 70.05 g of N2, (molar mass of N2 = 28.02 g/mol)
Use the dimensional analysis to get your answer
N2 + 3H2 ==> 2NH3moles N2 = 1.20 molesmoles NH3 formed = 1.20 moles N2 x 2 moles NH3/1 moles N2 = 2.40 moles NH3mass NH3 = 2.40 moles x 17 g/mole = 40.8 g NH3
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
The number of atoms is 45,166.10e23.
1 mole N2 = 22.4L 3.2L N2 x 1mol N2/22.4L = 0.14 mole N2
I assume you mean this reaction. N2 + 3H2 --> 2NH3 0.90 moles N2 (3 moles H2/1 mole N2) = 2.7 moles hydrogen gas needed =====================
Give the number of moles of N2 in 70.05 g of N2, (molar mass of N2 = 28.02 g/mol)
Use the dimensional analysis to get your answer
N2 + 3H2 ==> 2NH3moles N2 = 1.20 molesmoles NH3 formed = 1.20 moles N2 x 2 moles NH3/1 moles N2 = 2.40 moles NH3mass NH3 = 2.40 moles x 17 g/mole = 40.8 g NH3
If 5.0 moles of NH3 are produced 2.5 moles of N2 are used.
2 x 0.60 = 1.2 the reaction is N2 + 3H2 -> 2NH3 (1 mole of nitrogen N2 give 2 moles of NH3)
N2 + 3H2 -> 2NH3 If you have moles produced you can do it this way. 22.5 moles NH3 (3 moles H2/2 moles NH3) = 33.8 moles H2 needed -----------------------------------
Not necessarily. Some reactions do have the same number of moles, and some do not.Examples: NaCl + AgNO3 ==> NaNO3 + AgCl same # of moles N2 + 3H2 ==> 2NH3 different # of moles
50g/28g= 1.7857 moles
The reaction between nitrogen and hydrogen to form ammonia is: N2 + 3 H2 → 2 NH3 The above is the reaction for the Haber process in the industrial synthesis of ammonia. For a given proportion of 3 N2 to 2 H2 (or in ratio terms equivalent to 4.5 N2 to 3 H2), we see that H2 is the limiting reactant. Thus according to the stoichiometry of the reaction, 2 moles of H2 will form 1.33 moles of NH3.