300 moles of nitrogen equals 8404,2 g.
The density of nitrogen at 20 oc and 1 at is 1,251 g/cm3.
8404,2 g nitrogen equals 6 718 L.
1 kL = 1 000 L
So the volume of 300 moles N2 is 6,718 kL.
Without information on temperature and pressure, it is not possible.
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.
50g/28g= 1.7857 moles
The number of atoms is 45,166.10e23.
Use this formula. PV = nRT. Need to convert grams N2 to moles N2 and temperature Celsius to temperature Kelvin( add 273.15 )14.2 grams N2 ( 1mole N2/28.02 grams) = 0.507 moles N226 degrees C = 299.15 Kelvin(pressure)(10.0 liter) = (0.507 moles N2)(0.08206 Latm/molK)(299.15 K)= 1.24 atmospheres pressureThank you so much for your answer. I did end up figuring it out on my own.
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 =====================
9H2 + 3N2 ------> 6NH3 3 moles of N2 would be required.
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 -----------------------------------
50g/28g= 1.7857 moles
N2 + 3H2 --> 2NH3 You have been told, indirectly, that nitrogen limits and will drive the reaction. 3 moles N2 (2 moles NH3/1 mole N2) = 6 moles ammonia gas produced ========================
The answer is 0,0043 moles of N2.
N2(g) + 3H2-> 2NH3(g) This is the balanced equation Note the mole ratio between N2, H2 and NH3. It is 1 : 3 : 2 This will be important. moles N2 present = 28.0 g N2 x 1 mole N2/28 g = 1 mole N2 present moles H2 present = 25.0 g H2 x 1 mole H2/2 g = 12.5 moles H2 present Based on mole ratio, N2 is limiting in this situation because there is more than enough H2 but not enough N2. moles NH3 that can be produced = 1 mole N2 x 2 moles NH3/mole N2 = 2 moles NH3 can be produced grams of NH3 that can be produced = 2 moles NH3 x 17 g/mole = 34 grams of NH3 can be produced NOTE: The key to this problem is recognizing that N2 is limiting, and therefore limits how much NH3 can be produced.
The reaction of nitrogen with hydrogen to form ammonia is: N2 +3H2 = 2NH3 Therefore to make 10 moles of ammonia you need 5 moles N2 and 15 moles H2
The number of atoms is 45,166.10e23.