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, 1.85 g of NH3 reacts with 3.39 g of
O2.
1) How many grams of NO and of H2O form?
2) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Homework Answers
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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...
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, 2.05 g of NH3 reacts with 3.76 g of O2. How many grams of NO and of H2O form? Enter your answers numerically separated by a comma.
How many grams of NO and of H2O form? Enter your answers numerically separated by a...
How many grams of NO and of H2O form? Enter your answers numerically separated by a comma. How many grams of the excess reactant remain after the limiting reactant is completely consumed? 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, 1.50 g of NH3 reacts with 2.75 g of O2.
1) Ammonia, NH3, reacts with molecular oxygen, O2, to formnitric oxide, NO, and water:4NH3(g)...
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form
nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical
yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the
percent yield of the reaction
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO...
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NO B) O2 C) H2O D) no reagent is limiting E) NH3 What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? ___C7H14 + ___ O2 ---> ___ CO2 + __ H2O A) none of these B) 10...
The commercial production of nitric acid involves the following chemical reactions: (a) 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)⟶2NO2(g) (c)...
The commercial production of nitric acid involves the following chemical reactions: (a) 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)⟶2NO2(g) (c) 3NO2(g)+H2O(l)⟶2HNO3(aq)+NO(g) How many grams of ammonia must you start with to make 800.00 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric...
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is AHpxn for this reaction? 4NH3(g) + 5O2(g) -4NO(g) + 6H2O(9) Substance AH?f(kJ/mol) NH3(g) -46.3 NO(9) 90.3 H2O(9) -241.8 0 -1274.8 kJ/mol -904.4 kJ/mol 0 -240.2 kJ/mol 0 -197.8kJ 197.8 kJ/mol
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 produced by combining 67.5 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 many modern chemical proces...
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 58.5 g of each reactant? 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) mass: g H2O
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 +5O2 → 4NO + 6H2O
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 +5O2 → 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0g NH3 and 50.0g O2 are mixed and allowed to react: 1.87 mol 3.53 mol 1.57 mol 1.30 mol None of these
The first step in the Oswald process for producing nitric acid is 4NH+5o2- 4NO + 6H2O...
The first step in the Oswald process for producing nitric acid is 4NH+5o2- 4NO + 6H2O if 132g of ammonia reacts with 132g of oxygen A) how many grams of nk itric oxide(No) will be produced B) which compound is limiting reagent C) what is the % yield of this reaction if actual yield of NO is 67.Og?
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form
nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical
yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the
percent yield of the reaction
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is AHpxn for this reaction? 4NH3(g) + 5O2(g) -4NO(g) + 6H2O(9) Substance AH?f(kJ/mol) NH3(g) -46.3 NO(9) 90.3 H2O(9) -241.8 0 -1274.8 kJ/mol -904.4 kJ/mol 0 -240.2 kJ/mol 0 -197.8kJ 197.8 kJ/mol
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