Into an initially evacuated 20.0 L container maintained at 35.0°C were introduce
ID: 475061 • Letter: I
Question
Into an initially evacuated 20.0 L container maintained at 35.0°C were introduced 0.500 g of gaseous hydrogen and 3.00 g of gaseous nitrogen. A spark was used to initiate a reaction between hydrogen and nitrogen; gaseous ammonia was the sole product.
A) If the reaction occurred to the maximum possible extent, what was the pressure inside the container at the conclusion of the reaction? Assume all gases here behaved ideally.
B) What was the total mass of gas inside the container at the conclusion of the reaction?
Explanation / Answer
a]
N2 + 3H2 -----> 2NH3
T = 35C and V = 20 L
Mass of N2 = 3g
Mass of H2 = 0.5 g
Moles of N2 = 3/28 = 0.107
Moles of H2 = 0.5/2 = 0.25
N2 + 3H2 -----> 2NH3
0.0107 0.25 0
1 mole of N2 reacts with 3 moles of H2 and forms 2 moles of NH3
0.0107 moles of N2 reacts with 0.0107*3 = 0.0321 moles of H2
MOles of NH3 formed = 2*0.0107 = 0.0214
Moles of N2 left = 0
Moles of H2 left = 0.25 - 0.0321 = 0.2179
A]
PV = nRT
n = Total moles = 0.0214+0.2179 = 0.2393 [ Mole of N2 + Moles of NH3 ]
P = nRT / V = 0.302 atm
Pressure inside the container = 0.302 atm
B]
Mass of NH3 formed = 0.0214*17 = 0.3638 gms
Mass of H2 left = 0.2179*2 = 0.4358 gms
Total mass = 0.7996 gms
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