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29 Nov 2019

In the first step of the Ostwald process for the synthesis of nitric acid, ammonia is converted to nitric oxide by the high-temperature reaction 4NH3 (g) + 5O2 (g) --> 4NO (g) + 6H2O (g). (a) How is the rate of consumption of O2 related to the rate of consumption of NH3? (b) How is the rate of formation of NO related to the rate of consumption of NH3? (c) How is the rate of formation of H2O related to the rate of consumption of NH3?

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Deanna HettingerLv2

17 Dec 2019

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The first step in the Ostwald process for producing nitric acid is as follows:

4NH₃(g) + 5O₂(g) â 4NO(g) + 6H₂O(g).

If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

29.0%

32.9%

49.5%

61.8%

77.3%

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.

4NH3(g)+5O2(g)â¶4NO(g)+6H2O(g)

What is the maximum mass of H2O that can be produced by combining 21.6 g of each reactant?

STRATEGY:

Convert 21.6 g NH3 to moles, then find the corresponding amount of H2O.

Convert 21.6 g O2 to moles, then find the corresponding amount of H2O.

Identify the limiting reactant and calculate the mass of H2O produced.

Step 1: 21.6 g NH3 and excess O2 produce 1.90 mol H2O.

Step 2: 21.6 g O2 and excess NH3 produce 0.810 mol H2O.

Step 3: When 21.6 g NH3 and 21.6 g O2 are mixed, how many moles of H2O form?

(1) 1.90 + 0.810 mol H2O

(2) 0.810 mol H2O

(3) 1.90 mol H2O

Calculate the mass of H2O produced from the number of moles of H2O.

mass: [???] g H2O

bluewildebeest701

Ammonia reacts with oxygen to form nitric oxide and water vapor 4NH3 + 5O2 -> 4NO + 6H2O 1.What is the theoretical yield of water, in grams, when 0.210 Liters of 3.00 M NH3 and 31.0 g O2 are mixed and allowed to react? (1 mole NH3 = 17.04 g, 1 mole O2 = 32.00 g, 1 mole H2O = 18.02 g) 2.How much of the excess reagent in grams is left at the end of the reaction? Please be specific in each steps. Thanks

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