First make the reaction equation balanced for N-atoms (co-existant in both formula)
N2O5 + H2O --> 2 HNO3
So 1.02 mole HNO3 is produced from:
1.02 x 1 (N per HNO3) / 2 (N per N2O5) = 0.51 mol N2O5
Lets assume the reaction:
N2 + H2 -> NH3
Now to balance it:
1 N2 + 3 H2 -> 2 NH3
There is a 2/1 ratio for moles of NH3/N2
So 2 mol NH3 produced for every 1 mol of N2 reacted.
0.50 mol NH3 produced * (1 mol of N2 reacted / 2 mol NH3 produced) =
0.25 mol of N2 reacted.
Need balanced equation here.
N2 + 3H2 -> 2NH3
1.5 moles H2 (2 moles NH3/3 moles H2)
= 1.0 moles ammonia produced
=======================
0.5 [mol Ni(NO3)2] * 2 [mol N per mol Ni(NO3)2] = 1.0 mol N = 0.5 mol N2
There is one mole of N2 per mole of Ni(NO3)2; therefore there is one half mole of N2 in one half mole of Ni(NO3)2.
0.5 mole N2 <--------[ Answer ]
0,325 moles of nitrogen are involved in the reaction.
o.5
50 moles...
Hv
The mass of 7 050 moles of natural uranium is 238,02891 x 7 050.
316/.050 = 2320
4305 of them.
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.125 is thicker than .050
.050 inch.050 inch
5 050 000