Question
In: Chemistry
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 + 6H2O
__________ g H2O
Solutions
Expert Solution
4NH3 + 5O2 ----------------> 4NO + 6H2O
68 g 160 g 120 g 108 g
57.7 57.7 ??
here limiting reagent is O2. so product formed based on that.
160 g O2 ---------------> 108 g of H2O
57.7 g O2 ---------------> ??
mass of H2O produced = 57.7 x 108 / 160 = 39.0 g
mass of H2O = 39.0 g
queen_honey_blossom answered 2 years agoRelated Solutions
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. \(4NH_{3}(g)+5O_{2} -->
4NO+6H_{2}O(g)\) What is the maximum mass of H2O that can be
produced by combining 72.0 g of each reactant?
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
Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and...
Nitrogen dioxide is used industrially to produce nitric
acid, but it contributes to acid rain and photochemical smog. What
volume of nitrogen dioxide is formed at 791 torr
and 28.2°C by reacting 3.85
cm3of copper (d
= 8.95 g/cm3) with 240. mL of
nitric acid (d = 1.42
g/cm3, 68.0% HNO3 by mass)?
Cu(s) + 4HNO3(aq) →
Cu(NO3)2(aq) +
2NO2(g) + 2H2O(l)
______ L NO2
(A) Calculate the molarity of commercially available concentrated nitric acid reagent given the following data: Molecular...
(A) Calculate the molarity of commercially available
concentrated nitric acid reagent given the following data:
Molecular formula: HNO3
Molar mass = 63.01 g/mol
Purity/Reagent Concentrate: 70.9% (w/w)
Specific gravity @20 degrees Celsius = 1.423
(Hint: Using the specific gravity, calculate the mass of one
liter solution. Of this mass, only 70.9% is pure HNO3; the
remainder being water).
(B) To make 212 mL of 0.15 M solution of nitric acid, what
volume of the concentrated nitric acid will be needed?...
Redox Reactions: Less active metals like copper will reacti with concentrated nitric acid to produce nitric...
Redox Reactions: Less active metals like copper
will reacti with concentrated nitric acid to produce nitric oxide
gas and the Cu2+(aq) ion at 25C.
A) Write balanced chemical equation for this process.
6H+(aq) + 2HNO3(aq) +
3Cu(s) --> 3Cu2+(aq) +
2NO(g) + 4H2O (aq)
B) Evaluate change in E for the reaction in (a).
Consider the oxidation of ammonia to produce nitrogen dioxide. This reaction is used commercially in the...
Consider the oxidation of ammonia to produce nitrogen dioxide.
This reaction is used commercially in the production of nitric
acid.
4NH3 +
7O2 → 4NO2 +
6H2O
Which of the species in the above reaction either appears or
disappears the fastest?
Question 2 options:
A)
NH3
B)
O2
C)
NO2
D)
H2O
E)
The rates of appearance or disappearance are the same for all of
these species.
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.
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...
dentify the reaction or process used to manufacture a commercially made compound. It could be the...
dentify the reaction or process used to manufacture a
commercially made compound. It could be the pharmaceutical or
vitamin you previously posted about, or a pesticide, herbicide, or
active cleaning agent. It could even be a solvent used
and sold commercially. What we are focusing on for this
discussion is the reaction. Don’t forget to include a minimum of 1
APA formatted reference and approximately 250 words to discuss and
describe your reaction.
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