AND EQUILIBRIUMKINECalculating the reaction rate of one reactant from that of anotherDENitric 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 188, liters per second of dioxygen are consumed when thereaction is run at 266. °C and 0.42 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round youranswer to 2 significant digits.kgx10x 5?CheckExplanationPrivacy2019 McGraw-Hill Education. All Rights Reserved. Terms of Use

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Asked Nov 16, 2019
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Calculate the rate at which nitrogen monoxide is being reduced give your answer in kilograms per second round your answer to two significant digits. 

AND EQUILIBRIUM
KINE
Calculating the reaction rate of one reactant from that of another
DE
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 188, liters per second of dioxygen are consumed when the
reaction is run at 266. °C and 0.42 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your
answer to 2 significant digits.
kg
x10
x 5?
Check
Explanation
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2019 McGraw-Hill Education. All Rights Reserved. Terms of Use
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AND EQUILIBRIUM KINE Calculating the reaction rate of one reactant from that of another DE 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 188, liters per second of dioxygen are consumed when the reaction is run at 266. °C and 0.42 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. kg x10 x 5? Check Explanation Privacy 2019 McGraw-Hill Education. All Rights Reserved. Terms of Use

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Expert Answer

Step 1

Given,

Temperature of the reaction = 266°C = 266 + 273 K = 539 K

Pressure of the reaction = 0.42 atm = 42.55 K Pa

Volume of dioxygen = 188 litres

Gas Constant, R = 8.314 L K Pa K-1 mol-1

According to ideal gas equation,

PV nRT
PV
n =
RT
42.55 K Pa x 188 L
8.314 L K Pa mol K4 x 539 K
7999.4
4481.246 mol
n 1.7850 mol
n 0.001785 K mol
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PV nRT PV n = RT 42.55 K Pa x 188 L 8.314 L K Pa mol K4 x 539 K 7999.4 4481.246 mol n 1.7850 mol n 0.001785 K mol

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Step 2

Now the value of n=0.001785 K mol which is equal to the 17.8 g moles of nitrogen produced.

The reaction of the mixture is –

Therefore, the product of the...

4NH
50,4NO+ 6H,0
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4NH 50,4NO+ 6H,0

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