The industrial production of nitric acid (HNO3) is a multistep process. The first step is the...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here:
?NH3(g)+?O2(g)→?NO(g)+?H2O(g)
What volume of O2 at 912 mmHg and 41 ∘C∘C is required to
synthesize 24.5 mol of NO?
750 mmHg = 1 bar
R = 0.08314 L bar mol-1 K-1
Express your answer numerically in litres.
Homework Answers
4 NH3 + 5
O2
4 NO + 6 H2O
Number of moles of Oxygen needed = 5/4 × 24.5 mol = 30.625 mol
PV = n RT
912/750 bar × V = 30.625mol × 0.08314L.bar/K.mol × 314.15K
V = 657.8 L
Volume of O2 required = 658 L (Answer)
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The industrial production of nitric acid (HNO3) is a multistep
process. The first step is the...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 798 mmHg and 41 ∘C is required to synthesize 12.5 mol of NO? Express your answer to three significant figures and include the appropriate units.
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) Part A What volume of O2 at 684 mmHg and 41 ∘C is required to synthesize 19.0 mol of NO? Express your answer to three significant figures and include the appropriate units. volume of O^2=
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxi...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: NH3(g)+?O2(g)→?NO(g)+?H2O(g) What volume of O2 at 722 mmHg and 27 ∘C is required to synthesize 17.5 mol of NO?
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3 ) over a catalyst with excess oxygen (02) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH, (g)+?O2(g) +?NO(g)+?H2O(g) Part A What volume of O2 at 684 mmHg and 39 °C is required to synthesize 19.0 mol of NO? Express your answer to three significant figures and include the appropriate units. View Available Hint(s)...
What volume of O2 at 684 mmHg and 39 ∘C is required to synthesize 19.0 mol...
What volume of O2 at 684 mmHg and 39 ∘C is required to
synthesize 19.0 mol of NO?
Express your answer to three significant figures and include the
appropriate units.
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (02) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3 (g)+?02(g)?NO (g)+?H, O (g)
The first step in industrial nitric acid (HNO3) production is the catalyzed oxidation of ammonia (NH3)....
The first step in industrial nitric acid (HNO3) production is
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4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g).
When 0.0150 mol each of NH3(g) and O2(g) are placed in a 1.00 L
container at a certain temperature the N2(g) concentration at
equilibrium is 1.96x10-3 M. Fill in the following ICE table and
calculate the resulting KC.
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The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a...
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The first step in the industrial production of nitric acid is reacting ammonia with oxygen according to the unbalanced equation: NH3(g) + O2(g) → NO(g) + H2O(g) How many liters of NH3(g) at 850.oC and 5.00 atm are required to react with 32.0 g of O2? 0.811g of KClO3 is decomposed as follows: 2KClO3(s) → 2KCl(s) + 3O2(g) The O2 is collected over water at 28 oC and 765 torr. What is the volume of water displaced in this measurement,...
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Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first...
Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 988 liters per second of dioxygen are consumed when the reaction is run at 188. "C and 0.56 atm. Calculate the rate at...
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3 ) over a catalyst with excess oxygen (02) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH, (g)+?O2(g) +?NO(g)+?H2O(g) Part A What volume of O2 at 684 mmHg and 39 °C is required to synthesize 19.0 mol of NO? Express your answer to three significant figures and include the appropriate units. View Available Hint(s)...
What volume of O2 at 684 mmHg and 39 ∘C is required to
synthesize 19.0 mol of NO?
Express your answer to three significant figures and include the
appropriate units.
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (02) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3 (g)+?02(g)?NO (g)+?H, O (g)
The first step in industrial nitric acid (HNO3) production is
the catalyzed oxidation of ammonia (NH3). Without the catalyst the
following reaction predominates:
4NH3(g) + 3O2(g) ⇔ 2N2(g) + 6H2O(g).
When 0.0150 mol each of NH3(g) and O2(g) are placed in a 1.00 L
container at a certain temperature the N2(g) concentration at
equilibrium is 1.96x10-3 M. Fill in the following ICE table and
calculate the resulting KC.
NH3(9) 02(9) N2(9) H20(9) Initial (1) 015 mol mol .015 Number Number...
HOMWOPR Chapter II The Ideal Gas Law and Stoichiometry 14 of 15 Review Constants Periodic Table What volume of O, at 836 mmHg and 37 °C is required to synthesize 10.0 mol of NO? Express your answer to three significant figures and include the appropriate units. The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (Os) to produce nitrogen monoxide (NO) gas as...
Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 988 liters per second of dioxygen are consumed when the reaction is run at 188. "C and 0.56 atm. Calculate the rate at...
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