PV = nRT ⟹ n = PV/RT = 1 * 18.65 / (0.082 * 273.15) = 0.8321 moles.
18,65 L nitrogen is equivalent to 0,832 mol at 0 oC.
At STP 1 mole of any gas is contained in 22.4 L. So in 18.65 L, there will be 0.83 moles of nitrogen.
0.832 moles
The volume occupied by 3 moles of nitrogen gas will be different, depending on the temperature and pressure of the gas.
This depends on the mass of nitrogen contained in the balloon.
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
molar weight of N = 14 grams/mole 35.7 grams/14 grams/mole = 2.55 moles
There are 2 non bonding pairs in a nitrogen molecule
35.0 moles nitrogen (1 mole N/14.01 grams) = 2.50 moles nitrogen ----------------------------
4.561 / 28 = 0.163 moles of nitrogen.
15 grams of nitrogen are equal to 1,071 moles.
how many moles of sulfur are present in 3.4 moles of Al2(SO4)3
3 x 12 = 36 moles of Nitrogen atoms N or 18 moles of Nitrogen molecules N2
How many moles of atoms are contained in 382 g Co
1.38 moles of nitrogen equal16,62110876532.1023 atoms; the molecule of nitrogen is diatomic.
There are 29/14, or just over 2 moles of nitrogen in 19 grams.
10 moles of nitrogen dioxide are needed to react with 5,0 moles of water.
0.1868 moles
0.1868 moles
The volume occupied by 3 moles of nitrogen gas will be different, depending on the temperature and pressure of the gas.