Question
In: Chemistry
One of the steps in the commercial process for converting ammonia to nitric acid is the...
One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH3 to NO:
NH.3 (g) + (g) NO (g) H20(g)
In a certain experiment, 2.00 grams of ammonia reacts with 2.50
grams of o2. What is the limiting reagent? How many grams of NO and
H2O form? How many grams of the excess reactant remain after the
limiting reactant is completely consumed? Show by your calculations
that the Law of Conservation by mass is not violated.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
One of the steps in the commercial process for converting ammonia to nitric acid is the...
One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH3 to NO:
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)
In a certain experiment, 1.20 g of NH3 reacts with 2.20 g of
O2.
a) How many grams of NO and of H2O form? Enter your answers
numerically separated by a comma.
b) How many grams of the excess reactant remain after the
limiting reactant is completely consumed? Express your answer in
grams to three significant figures.
Question 14 One of the steps in the commercial process for converting ammonia to nitric acid...
Question 14
One of the steps in the commercial process for converting
ammonia to nitric acid is the conversion of NH3 to NO:
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)
In a certain experiment, 2.10 g of NH3 reacts with 3.85 g of
O2.
Part B
How many grams of NO and of H2O form?
Enter your answers numerically separated by a comma.
mNO,mH2O =
g
Part C
How many grams of the excess reactant remain after the limiting
reactant is completely consumed?
m =
one of the steps in the manufacture of nitric acid is the oxidation of ammonia shown...
one of the steps in the manufacture of nitric acid is the
oxidation of ammonia shown in this equation: 4NH 3 (g) + 5O 2 (g) →
4NO (g) + 6H 2 O (g).
if 43.0 kg of NH3 reacts with 35.4 Kg of O2, what mass of NO
forms?
In a titration of 46.24 mL of 0.3359 M ammonia with 0.3359 M aqueous nitric acid,...
In a titration of 46.24 mL of 0.3359 M ammonia with 0.3359 M
aqueous nitric acid, what is the pH of the solution when 46.24 mL
of the acid have been added?
In a titration of 44.86 mL of 0.3356 M ammonia with 0.3356 M aqueous nitric acid,...
In a titration of 44.86 mL of 0.3356 M ammonia with 0.3356 M
aqueous nitric acid, what is the pH of the solution when 44.86 mL
of the acid have been added?
Ammonia gas enters the reactor of a nitric acid plant mixed with 30% more dry air...
Ammonia gas enters the reactor of a nitric acid plant mixed with
30% more dry air than is required for the complete conversion of
the ammonia to nitric oxide and water vapor. If the gases enter the
reactor at 75 ◦ C (167 ◦ F), if conversion is 80%, if no side
reactions occur, and if the reactor operates adiabatically, what is
the temperature of the gases leaving the reactor? Assume ideal
gases.
The first reaction in the Ostwald process for the production of nitric acid involves the combustion...
The first reaction in the Ostwald process for the production of
nitric acid involves the combustion of ammonia
4NH3(g)+5O2(g)=4NO(g)+6H2O(g)
a) Estimate ΔH^o (in kJ) for this reaction using average bond
energies.
b) Calculate ΔH^o (in kJ) for this reaction using standard heats
of formation.
c) Briefly explain why the value for ΔH^o, calculated using
average bond energies, is only considered to be an estimate of the
standard enthalpy change for the reaction
The following sequence of reactions occurs in the commercial production of aqueous nitric acid. 4 NH3(g)...
The following sequence of reactions occurs in the commercial
production of aqueous nitric acid. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6
H2O(l) ΔH = −1166.0 kJ/mol 2 NO(g) + O2(g) → 2 NO2(g) ΔH = −116.2
kJ/mol 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) ΔH = −137.3 kJ/mol
Determine the total energy change (in kJ) for the production of one
mole of aqueous nitric acid by this process. _____ kJ
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in...
The Ostwald process is used commercially to produce nitric acid,
which is, in turn, used in many modern chemical processes. In the
first step of the Ostwald process, ammonia is reacted with oxygen
gas to produce nitric oxide and water. What is the maximum mass of
H2O that can be produced by combining 62.6 g of each reactant?
4NH3(g) + 5O2 (g) > 4NO (g) +6H2O(g)
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in...
The Ostwald process is used commercially to produce nitric acid,
which is, in turn, used in many modern chemical processes. In the
first step of the Ostwald process, ammonia is reacted with oxygen
gas to produce nitric oxide and water. What is the maximum mass of
H2O that can be produced by combining 57.7 g of each reactant?
what is the maximum mass of H2O that can be produced by
combining 57.7g of each reactant?
4NH + 5O2 --------> 4NO...
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