Question

One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown...

One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation:

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

If 47.0 kg of NH3 reacts with 120. kg of O2, what mass of NO is formed?

Homework Answers

Answer #1

Molar mass of NH3,

MM = 1*MM(N) + 3*MM(H)

= 1*14.01 + 3*1.008

= 17.034 g/mol

mass(NH3)= 47.0 Kg = 47000 g

number of mol of NH3,

n = mass of NH3/molar mass of NH3

=(47000.0 g)/(17.034 g/mol)

= 2.759*10^3 mol

Molar mass of O2 = 32 g/mol

mass(O2)= 120 Kg = 120000 g

number of mol of O2,

n = mass of O2/molar mass of O2

=(120000.0 g)/(32 g/mol)

= 3.75*10^3 mol

Balanced chemical equation is:

4 NH3 + 5 O2 ---> 4 NO + 6 H2O

4 mol of NH3 reacts with 5 mol of O2

for 2759.1875 mol of NH3, 3448.9844 mol of O2 is required

But we have 3750 mol of O2

so, NH3 is limiting reagent

we will use NH3 in further calculation

Molar mass of NO,

MM = 1*MM(N) + 1*MM(O)

= 1*14.01 + 1*16.0

= 30.01 g/mol

According to balanced equation

mol of NO formed = (4/4)* moles of NH3

= (4/4)*2759.1875

= 2759 mol

mass of NO = number of mol * molar mass

= 2.759*10^3*30.01

= 8.28*10^4 g

Answer: 8.28*10^4 g

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Nitric Oxide is made from the oxidation of ammonia. What mass of nitric oxide can be...
Nitric Oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2? 4 NH3(g) + 5 O2(g) --> 4 NO(g) + 6 H2O(g)
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, 1.60 g of NH3 reacts with 2.93 g of O2. How many grams of the excess reactant remain after the limiting reactant is completely consumed?
1) One of the steps in the commercial process for converting ammonia to nitric acid is...
1) 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) How many grams of NO and of H2O form? Enter your answers numerically separated by a comma. In a certain experiment, 2.10 g of NH3 reacts with 3.85 g of O2. 2) 2C8H18(g)+25O2(g)→16CO2(g)+18H2O(g) How many moles of water are produced in this reaction? After the reaction, how much octane is left? 3) 3H2(g)+N2(g)→2NH3(g) 1.71 g H2 is...
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 874 mmHg and 33 ∘C is required to synthesize 18.0 mol of NO?
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 684 mmHg and 27 ∘C is required to synthesize 20.0 mol of NO?
Modern processes for the production of nitric acid are based upon the oxidation of ammonia synthesized...
Modern processes for the production of nitric acid are based upon the oxidation of ammonia synthesized via the Haber reaction. The first step of the oxidation process is the reaction of NH3 with O2 over a platinum catalyst to produce nitric oxide: 4NH3 + 5O2 ------> 4NO + 6H2O Under a given set of reactor conditions, 90% conversion of NH3 is obtained with a feed of 40 moles/hr NH3 and 60 moles/hr O2. (a) What is the limiting reactant? (b)...
The Ideal Gas Law and Stoichiometry The industrial production of nitric acid (HNO3) is a multistep...
The Ideal Gas Law and Stoichiometry 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 836 mmHg and 27 ∘C is required to synthesize 10.5 mol of NO? Express your answer to three significant figures and include the appropriate units.
The Ideal Gas Law and Stoichiometry The industrial production of nitric acid (HNO3) is a multistep...
The Ideal Gas Law and Stoichiometry 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 836 mmHg and 27 ∘C is required to synthesize 10.5 mol of NO? Part B What volume of H2O(g) is produced by the reaction under...
In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas...
In the manufacture of nitric acid, ammonia and preheated air are mixed to form a gas containing 10 mole% NH3 at 600oC. (The ammonia is not preheated, since if it were, it will decompose to N2 and H2). The mixture is then catalytically oxidized to form NO2, which is absorbed in water to form HNO3. If ammonia enters the gas blending (mixing) unit at 25oC at a rate of 520 kg/h, and heat is lost from the mixer to its...
Ammonia NH3 chemically reacts with oxygen gas O2 to produce nitric oxide NO and water H2O...
Ammonia NH3 chemically reacts with oxygen gas O2 to produce nitric oxide NO and water H2O . What mass of nitric oxide is produced by the reaction of 1.3g of oxygen gas? Be sure your answer has the correct number of significant digits.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT