Question

For the unbalanced reaction H2​(g)+NO(g) ---> H2​O(g)+N2​(g): the initial concentrations are 5.25 M H2, 9.00 M...

For the unbalanced reaction H2​(g)+NO(g) ---> H2​O(g)+N2​(g):

the initial concentrations are 5.25 M H2, 9.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.75 M.

A) Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation.

B) Calculate the value of K under the reaction conditions at equilibrium.

0 0
Add a comment Improve this question Transcribed image text
Answer #1

H2(g) + NO(g) ----------- H2O(g) + N2(g)

The balanced equation i s

               2 H2(g) + 2NO(g) ----------- 2H2O(g) + N2(g)

Initial concentration of H2= 5.25M

                                  [NO] = 9.00M

at equilibrium [N2] = 1.75M

a)

The balanced equation is

                                      2 H2(g) + 2NO(g) ----------- 2H2O(g) + N2(g)

B)

                                    2 H2(g) + 2NO(g) ----------- 2H2O(g) + N2(g)

Initial                               5.25         9.00                    0               0

chnage                            -2x           -2x                     +2x             +x

equilibrium                  5.25-2x        9.00-2x               +2x               +x ( 1.75)

according to given data

at equilibrium [N2] = x= 1.75M

x= 1.75M

at equilibrium

[H2] = 5.25 - 2x = 5.25 - 2(1.75) = 1.75M

[NO] = 9.00-2x= 9.00 - 2(1.75) = 5.5M

[H2O] = 2x = 2 x1.75 = 3.5M

K= [H2O]^2 [N2]/ [H2[^2[NO]^2

K = ( 3.5)^2 x 1.75 / (1.75)^2 x(5.5)^2

K= 21.4375/92.641

K = 0.231

Equilibrium constant = K = 0.231.

Add a comment
Know the answer?
Add Answer to:
For the unbalanced reaction H2​(g)+NO(g) ---> H2​O(g)+N2​(g): the initial concentrations are 5.25 M H2, 9.00 M...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Calculate Kc for the following reaction given the following equilibrium concentrations of H2(g) = 1.60 M...

    Calculate Kc for the following reaction given the following equilibrium concentrations of H2(g) = 1.60 M CO(g) = .0030 M, and H2O(g) = 0.030 M. C(s) + H2O(g) =  CO(g) + H2(g) (Hint: You DO include H2O(g) in the equilibrium expression) K = ? Save Answer Calculate K, for the following reaction given the following equilibrium concentrations of H2(9) = 1.60 M COO) = .0030 M, and H,00 = 0.030 M. Co+H,09 = COO + H2(9) (Hint: You Do include H,0...

  • For the reaction H_2(g) + S(g) H_2S(g) the initial concentrations are 0.060 M H_2, 0.080 MS,...

    For the reaction H_2(g) + S(g) H_2S(g) the initial concentrations are 0.060 M H_2, 0.080 MS, and no H_2S. At equilibrium, [H_2] = 0.010 M. Calculate the concentrations of S and H_2S at equilibrium. (Be sure to give your answers to three decimal places.) M S M H_2 S Calculate the value of K under the reaction conditions at equilibrium. (Be sure your answer has the appropriate number of significant figures.)

  • For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations...

    For the reaction N2(g) + 3H2(g) = 2NH3(g) what is the value of Ke at 500°C if the equilibrium concentrations are as follows: [H2] = 0.40 M, (N2) = 0.40 M, and (NH3) = 1.9 M Express the equilibrium constant to two significant figures. V AE OE ? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Set up the equilibrium-constant expression for this reaction using the equilibrium concentrations. The product concentrations a the reactant concentrations are...

  • 1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...

    1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...

  • Consider the following reaction: N2(g)+3H2(g)⇌2NH3(g) Complete the following table. Assume that all concentrations are equilibrium concentrations...

    Consider the following reaction: N2(g)+3H2(g)⇌2NH3(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (K) [N2] [H2] [NH3] [Kc] 500 0.115 0.105 0.439 − 575 0.105 M − 0.128 M 9.6 775 0.130 M 0.145 M − 0.0584 Find Kc at 500 K. Find [H2] at 575 K. Find [NH3] at 775 K.

  • Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations...

    Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<---                    ---->2HI(g)

  • 1. The initial concentrations of reactants and products for this reaction are given below. N2(g)   +  ...

    1. The initial concentrations of reactants and products for this reaction are given below. N2(g)   +   O2(g)  ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...

  • The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2...

    The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2 NH3(g)       Kc=? Write the equilibrium constant expression (Kc) for this reaction. Calculate the value of Kc at 500. K for the formation of ammonia in part a) using the following measured concentrations for the equilibrium mixture: [N2] = 3.0 x 10-­‐2  M; [H2] = 3.7 x 10-­‐2  M; [NH3] = 1.6 x 10-­‐2  M.                                                                                [1.7 x 102] Now, calculate the value of Kc for the formation of...

  • 2.1 For the reaction N2(g) + C2H2(g) == 2HCN(g) K=0.0324 What are the equilibrium concentrations of...

    2.1 For the reaction N2(g) + C2H2(g) == 2HCN(g) K=0.0324 What are the equilibrium concentrations of all species present if the initial concentrations are [N2] = [C2H2] = [HCN] = 2.50 M?

  • The following reaction 2NO(0) + 2H2 (g) № (g) + 2 HaO (g) H2/0000 M quilbrium constant, Ke, for t...

    the following reaction 2NO(0) + 2H2 (g) № (g) + 2 HaO (g) H2/0000 M quilbrium constant, Ke, for the reaction. Initially, a mixture of 0.300 M NO, 0.100 M NOwas found to beg,062-м. D.ig2 the value of the brium (init h N2)t eubrhum the conentreton dr H20 was allowed to reach equilibrium ( 0-200 8) Consider the following reaction. HSO.. (aq) + H2O (I) → HO. (aq) + SO2-(aq) The initial concentrations are [HSO門-0.3000 M, [HO+]s 0.050 M. [SO...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT