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.
Homework Answers
Add Answer to:
How many grams of NO and of H2O form?
Enter your answers numerically separated by a...
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?
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.
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...
How many grams of H2O can be prepared from 11.25grams of NH3 and 56.03g of O2in...
How many grams of H2O can be prepared from 11.25grams of NH3 and 56.03g of O2in the following equation? 4NH3(g) + 5O2(g) arrow 4NO+ 6H2O(g)
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
1. How many moles of MgS2O3 are in 225 g of the compound? 2. Determine the...
1. How many moles of MgS2O3 are in 225 g of the compound? 2. Determine the empirical formula for a compound that is 64.8% C, 13.6% H, and 21.6% O by mass. 3.A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? 4.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...
If the reaction consumes (uses up) 31.7 moles of ammonia, how many grams of water will...
If the reaction consumes (uses up) 31.7 moles of ammonia, how many grams of water will be produced using the following equation? 4NH3 + 5O2 g 4NO + 6H2O
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.
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
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
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