Question

The reaction N2(g) + 3H2(g) ⇌ 2NH3(g) has KC = 0.500 at 400*C. Write the reaction...

The reaction N2(g) + 3H2(g) ⇌ 2NH3(g) has KC = 0.500 at 400*C. Write the reaction quotient (QC) expression including the “i” subscripts. Then, find the value for QC if [N2] = 0.015 M, [H2] = 0.12 M, and [NH3] = 0.00054 M. Compare this value with KC and determine which direction the reaction will go towards.

Homework Answers

Answer #1

Kc is the equilibrium constant for a reaction. It depends on the concentration of reactants and products when the equlibrium is reached.

Qc is called reaction quotient. It the ratio of concentration of product to reactants raised to their powder at any stage during the reaction.

Given, [NH3]=0.00054M [N2] = 0.015M

[H2]=0.12M

Then Qc= [NH3]i2/ [N2]i[H2]i3

Qc= (0.00054*0.00054)/(0.015*0.12*0.12*0.12)

Qc= 0.01125

Given Kc= 0.500

Since, Qc < Kc. The reaction shifts in the forward direction.

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) Consider the following reaction where Kc = 0.159 at 723 K. N2(g) + 3H2(g) 2NH3(g)...
A) Consider the following reaction where Kc = 0.159 at 723 K. N2(g) + 3H2(g) 2NH3(g) A reaction mixture was found to contain 4.94×10-2 moles of N2(g), 4.07×10-2 moles of H2(g) and 6.19×10-4 moles of NH3(g), in a 1.00 liter container. The reaction quotient, Qc, equals __________. The reaction__________________ A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium. B) Consider the following reaction where Kc...
kc= 0.00592 for the reaction below at 351 K. N2 (g) + 3H2 (g) <----> 2NH3...
kc= 0.00592 for the reaction below at 351 K. N2 (g) + 3H2 (g) <----> 2NH3 (g). What is Kc at 351 K for the reaction: 1/3 N2 (g) +H2 (g)<--->2/3 NH3 (g)
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture...
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture of 1.0 mol each of N2, H2, and NH3 are placed into a 1.0 L flask and allowed to come to equilibrium at 500.0 C. Kp at this temperature is 1.45 x 10-5 atm-2. A.) What is the value of Kc at this temperature? irst find the relationship between Kc and Kp in terms of RT. Then substitute T = 773K and R =...
Consider the reaction, N2(g) + 3H2(g) Picture 2NH3(g). Kc = 4.2 at 600 K. What is...
Consider the reaction, N2(g) + 3H2(g) Picture 2NH3(g). Kc = 4.2 at 600 K. What is the value of Kc for 4 NH3(g) Picture 2N2(g) + 6H2(g)?
The chemical reaction N2(g) + 3H2(g) 2NH3(g) is carried out at 400. K. Assume the partial...
The chemical reaction N2(g) + 3H2(g) 2NH3(g) is carried out at 400. K. Assume the partial pressures of N2(g), H2(g), and NH3(g) are 1.0, 4.2, and 63 atm, respectively. The value of Kp = 54 at 700. K. for this reaction. (a) Calculate the reaction free energy. (b) Indicate whether this reaction mixture is likely to form reactants, is likely to form products, or is at equilibrium.
Write the equation for the reaction quotient Q for a reaction. N2(g) +3H2(g)--- 2NH3(g) What is...
Write the equation for the reaction quotient Q for a reaction. N2(g) +3H2(g)--- 2NH3(g) What is the value of Q when partial pressure of nitrogen is 0.20 bar,for hydrogen 0.40 bar and for ammonium 0.61 bar?
N2(g) + 3H2(g) →2NH3(g) If there is 10.02 g N2 and excess H2 present, the reaction...
N2(g) + 3H2(g) →2NH3(g) If there is 10.02 g N2 and excess H2 present, the reaction yields 9.47 g NH3. Calculate the percent yield for the reaction
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g)...
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kc= 1.2 at 375 °C. If the starting concentrations are [H2] = 0.76 M, [N2] = 0.60 M, and [NH3] = 0.48 M, at equilibrium which gases will have increased in concentration and which will have decreased in concentration? a. H2 b. N2 c. NH3 part b When solid sodium bicarbonate is heated the following decomposition reaction occurs: 2NaHCO3(s) ⇌...
consider the reaction: N2(g)+3h2 <-------> 2NH3(g). Kp for this reactin at 723K is 4.51x10-5. indicate in...
consider the reaction: N2(g)+3h2 <-------> 2NH3(g). Kp for this reactin at 723K is 4.51x10-5. indicate in each reation is at equilibrium. if not, indicate in which direction the reaction must proceed to reach equilibrium. a. 100 atm NH3(g), 30 atm N2(g), 500 atm H2(g) b. 2.0M NH3(g), 3.0M N2(g) , 5.0 H2(g) must show work to recieve full credit on hw assignment!
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4...
consider the following reaction: 2NH3 (g) <=> N2 (g) + 3H2 (g) if 7.92 x 10-4 moles of NH3, 0.336 moles of N2 and 0.287 moles of H2 are at equilibrium in a 10.2 L container at 884 K, the value of the equilibrium, Kp, is _