Question

If the reaction N2 (g) + 3 H2 (g) --> 2 NH3 (g) has the concentrations...

If the reaction N2 (g) + 3 H2 (g) --> 2 NH3 (g) has the concentrations 0.55 M for nitrogen, 0.75 M for hydrogen and 0.25 M for ammonia gas, what is the Kc? Show all work. Does this mean that there are more reactants or products at equilibrium? Explain how you determined that.

Homework Answers

Answer #1

Kc is the equilibrium constant; Kc= [products]/[reactants]

For the above reaction, Kc = [NH3]2 / [N2] [H2]3  

[NH3] = 0.25 M

[N2] = 0.55 M

[H2] = 0.75 M

Hence  Kc = [0.25 ]2 / [0.55 ] [0.75]3 = 0.0625 / 0.55 x 0.42 = 0.269

If Kc is larger than 1(Kc > 1) the mixture contains more of the products.

If Kc is less than 1(Kc < 1), the mixture contains more of the reactants.

If Kc is equal to 1(Kc = 1), the amounts of products and reactants are almost the same.

Here Kc < 1, hence there is more reactants than the products in the mixture.

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
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.
A: 2 NH3 (g) + 46 kJ <-> N2 (g) + 3 H2 (g) For the...
A: 2 NH3 (g) + 46 kJ <-> N2 (g) + 3 H2 (g) For the reaction at equilibrium given above, give 2 ways that you can shift the equibrium to the left. B: 2 NH3(g) + 46 kJ <-> N2(g) + 3 H2(g) For the reaction at equilbrium given above, calculate the numeric value of Kc if the concentrations at equilibrium are 0.50 M NH3(g) , 0.44 M N2(g), and 0.20 M H2(g). C: 2 NH3(g) + 46 kJ...
Please show your work! a) Write the equlibrium equation for the following reaction. N2 (g) +...
Please show your work! a) Write the equlibrium equation for the following reaction. N2 (g) + 3 H2 (g) <===> 2 NH3 (g) b) An equilibrium mixture at 500 K has the following concentrations : [N2] = 3.0 x 10-2 M, [H2] = 3.7 x 10-2 M, [NH3] = 1.6 X 10-2 , calculate the equilibrium constant, Kc. c) Calculate the Kp for this reaction. d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to...
The reaction N2 + 3 H2----> 2 NH3 is used to produce ammonia. When 450.0 g...
The reaction N2 + 3 H2----> 2 NH3 is used to produce ammonia. When 450.0 g of hydrogen was reacted with nitrogen, the percent yield you achieved was 30.8%. What was the mass of ammonia produced?
2. At 450°C, ammonia gas will decompose according to the following equation: 2 NH3 (g) ...
2. At 450°C, ammonia gas will decompose according to the following equation: 2 NH3 (g)  N2 (g) + 3 H2 (g) Kc = 4.50 at 475˚C An unknown quantity of NH3 is placed in a reaction flask (with no N2 or H2) and is allowed to come to equilibrium at 475°C. The equilibrium concentration of H2 is then determined to be 0.252 M. Determine the initial concentration of NH3 placed in the flask
(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for...
(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for an isothermal, isobaric flow system with equimolar (or equal molar) feeds of N2 & H2. (b) If the entering total pressure is 16.4 atm and the entering temperature is 1727 oC, calculate the concentration of hydrogen and nitrogen entering the reactor. (c) Plot the gas composition (molar fractions) as a function of the conversion. Is there anything worth noticing? Can you explain it? What...
Ammonia equilibrium N2 (g) + 3 H2 (g) <-> 2 NH3 (g) is at equilibrium when...
Ammonia equilibrium N2 (g) + 3 H2 (g) <-> 2 NH3 (g) is at equilibrium when additional nitrogen is added under specific conditions, where T and P held constant, further dissociation of ammonia occurs A) Explain why. B) What conditions are needed? C) Why would adding more H2 produce the same result? This is Physical Chemistry homework. Thank you!
Consider the following reaction: 2 NO(g) + 5 H2(g) ? 2 NH3(g) + 2 H2O(g) Which...
Consider the following reaction: 2 NO(g) + 5 H2(g) ? 2 NH3(g) + 2 H2O(g) Which set of solution maps would be needed to calculate the maximum amount of ammonia (NH3), in grams, that can be synthesized from 45.8 g of nitrogen monoxide (NO) and 12.4 g of hydrogen (H2)? I. g NO ? mol NO ? mol NH3 ? g NH3 II. g H2 ? mol H2 ? mol NH3 ? g NH3 III. g NO ? mol NO...
Use the balanced equation for the exothermic reaction, N2 (g) + 3 H2 (g)----->2 NH3 (g),...
Use the balanced equation for the exothermic reaction, N2 (g) + 3 H2 (g)----->2 NH3 (g), to answer the 4 questions below. In which direction will the system shift when hydrogen is added? _____________ In which direction will the system shift when nitrogen is removed? _____________ In which direction will the system shift when ammonia is added? _____________ In which direction will the system shift when the temperature is increased? _____________
Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures. 3...
Ammonia, NH3, is produced from the reaction of gaseous nitrogen and hydrogen at high temperatures. 3 H2 (g) + N2 (g)  → 2 NH3 (g) For the reaction of 3.77 g of H2 with 8.66 g of N2, you determined that 21.2 g and 10.5 g of ammonia could be produced, respectively. In the laboratory, you reacted these masses of H2 and N2 and collected 7.70 g of NH3. What is the percentage yield of this reaction to the correct number...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT