a.) How many grams of NH3 can be produced from 4.19 mol of N2
and excess H2? Express your answer numerically in grams.
b.) How many grams of H2 are needed to produce 11.70g of NH3
c.) How many molecules (not moles) of NH3 are produced from
2.64x10^-4 g of H2
a) How many grams of NH3 can be produced from 4.75
mol of N2 and excess H2?
b) How many grams of H2 are needed to produce 11.85 g
of NH3?
c) How many molecules (not moles) of NH3 are produced
from 7.98x10-4 g of H2?
d) What mass of HCl in grams is neutralized by a dose of milk of
magnesia containing 3.55 g Mg(OH)2?
3H2(g)+N2(g)?2NH3(g)
How many grams of NH3 can be
produced from 3.23mol of N2 and excess H2.
How many grams of H2 are needed to produce 13.85g of NH3?
How many molecules (not moles) of NH3 are produced from 6.68
How many moles of NH3 can be produced when 11.00 mol H2 react
with 5.00 mol N2?
_________mol NH3
How many moles of each reactant are left over? Note that at
least one must disappear.
______mol H2 remain
_______mol N2 remain
Assume that you have 1.48 mol of H2 and 3.47 mol of N2. How many
grams of ammonia (NH3)can you make, and how many grams of which
reactant will be left over?
3H2+N2→2NH3
Part A
mNH3 =
g
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Part B
mH2 =
g
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Part C
mN2 =
g
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A mixture of 0.09581 mol of C2H4, 0.02766 mol of N2, 0.04516 mol
of NH3, and 0.08098 mol of C6H6 is placed in a 1.0-L steel pressure
vessel at 731 K.
The following equilibrium is established:
3 C2H4(g) + 1 N2(g) 2 NH3(g) + 1 C6H6(g)
At equilibrium 0.006932 mol of N2 is found in the reaction
mixture.
(a) Calculate the equilibrium partial pressures of C2H4, N2,
NH3, and C6H6.
Peq(C2H4) = .
Peq(N2) = .
Peq(NH3) = .
Peq(C6H6)...