Question

For the reaction below (an undesired side reaction in the industrial production of nitric acid), if...

For the reaction below (an undesired side reaction in the industrial production of nitric acid), if you begin by adding 0.0150 moles of both NH3 and O2 to a 1.00 L reaction vessel, and once equilibrium is established you have a nitrogen concentration of 0.00196 M, what is the value for Kc?

4 NH3 (g)   + 3 O2 (g)   <-->   2 N2 (g) +   6 H2O (g)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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?
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...
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2HNO3 (aq)...
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2HNO3 (aq) + NO (g) → 3NO2 (g) + H2O (l) At a certain temperature, a chemist finds that a 9.5L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 15.5g NO 16.6g NO2 22.5g H2O 189.0g Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to...
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.
Nitric oxide reacts with oxygen to give nitrogen dioxide, an important reaction in the Ostwald process...
Nitric oxide reacts with oxygen to give nitrogen dioxide, an important reaction in the Ostwald process for the industrial synthesis of nitric acid: 2NO(g)+O2(g)?2NO2(g) Part A If Kc=6.9
A 2 L reaction vessel contains NH3, N2 and H2 at equilibrium at a certain temperature....
A 2 L reaction vessel contains NH3, N2 and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [NH3] = 0.25 M, [N2] = 0.11 M and [H2] = 1.91 M. Calculate the equilibrium constant Kc for the synthesis of ammonia as described in the following reaction. N2 (g) + 3H2 (g) 2 NH3 (g) If 0.12 moles of N2 is then added to the reaction flask. Calculate the new equilibrium concentrations.
The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) <---> NH3(g)...
The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) <---> NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.338 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [arrows used to indicate rxn]
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K:...
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.75 mol of C, 14.1 mol of H2O, 3.60 mol of CO, and 8.50 mol of H2, what is the reaction quotient Q? 2) The following reaction was performed in a sealed vessel at 782 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.65M and...
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT