If 8.00 L of water vapor at 50.2 °C and 0.121 atm reacts with excess iron, how many grams of iron(III) oxide will be produced?
2Fe + 3H2O ----- Fe2O3 +3H2
1st find the mol of Fe reacted
we have:
P = 0.121 atm
V = 8.0 L
T = 50.2 oC
= (50.2+273) K
= 323.2 K
find number of moles using:
P * V = n*R*T
0.121 atm * 8 L = n * 0.08206 atm.L/mol.K * 323.2 K
n = 3.65*10^-2 mol
from reaction,
mol of Fe2O3 formed = (1/2)*mol of Fe reacted
= (1/2)*3.65*10^-2 mol
= 1.825*10^-2 mol
Molar mass of Fe2O3 = 2*MM(Fe) + 3*MM(O)
= 2*55.85 + 3*16.0
= 159.7 g/mol
we have below equation to be used:
mass of Fe2O3,
m = number of mol * molar mass
= 1.825*10^-2 mol * 159.7 g/mol
= 2.915 g
Answer: 2.92 g
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