Chemistry - Correction

posted by .

I just wanted to be sure if my answers make any sense.

Thank you;

For the reaction of ammonia:

N2(g) + 3H2(g) --> 2NH3(g)

suppose equilibrium has been established. Explain how and why the position of equilibrium will shift in response to the following changes:

(a) Additional nitrogen is added to the system
(b) Ammonia is removed from the system as it forms
(c) The pressure on the system is increased

(A) I think it will shift right, because we add more reactant so we need to make more product.

(B) If ammonia is removed it will shift to the left to compensate for that loss

(C) If the pressure is increased then the reaction it will shift right because we have less space, so it shifts to where there's less moles.

  • Chemistry - Correction -

    I answered this just now at the original; I'm a little late catching up from yesterday.
    A is right.
    C is right.
    B is not right.
    If NH3 is REMOVED as it is formed then the reaction must shift to the right in order to replace that which has been removed.

  • Chemistry - Correction -

    Thanks Bob!

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    A container initially has 0.0186 M ammonia at a certain temperature. When the system reaches equilibrium the concentration of ammonia is 0.0035 M. Calculate Kc for the following reaction as written. N2(g) + 3H2(g) --> 2NH3(g)
  2. chemistry

    I am given the following reaction: 2NH3(g) -------> N2(g) + 3H2(g) My question is: 6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If …
  3. chemistry

    I am given the following reaction: 2NH3(g) -------> N2(g) + 3H2(g) My question is: 6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If …
  4. chemistry

    I am given the following reaction: 2NH3(g) -----> N2(g) + 3H2(g) 6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium …
  5. Chemistry

    I just wanted to be sure if my answers make any sense. Thank you; For the reaction of ammonia: N2(g) + 3H2(g) --> 2NH3(g) suppose equilibrium has been established. Explain how and why the position of equilibrium will shift in response …
  6. Chemistry

    For the reaction 2NH3(g) 3H2(g) N2(g) at 472oC equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37x10^_8 M. What is the equilibrium constant for the reverse reaction?
  7. Chemistry

    N2(g)+3H2(g) -> 2NH3(g)+ 22000 cal Consider the reaction is at equilibrium. Explain how the equilibrium is shifted when a. more N is added b. more H is added c. ammonia is removed
  8. Chemistry

    For the formation of ammonia, the equilibrium constant is known to be 5.2 × 10^−5 at 25◦C. After analysis, it is determined that [N2] =3M and [H2]=0.8M, both at equilibrium. How many grams of ammonia are in the 10L reaction …
  9. chem

    For the reaction: N2+3H2 <-----> 2NH3 1.000 mol N2 and 1.000 mol H2 are placed in a 1.000 L container and allowed to establish equilibrium. When equilibrium is established the [N2] =0.921M. Calculate the equilibrium concentrations …
  10. chem

    For the reaction: N2+3H2<--->2NH3 4.000 mol N2, 2.000 mol H2, and 6.000 mol NH3 are placed in a 2.000 L container and allowed to reach equilibrium. When equilibrium is established the [H2]=2.77 M. Calculate the equilibrium concentrations …

More Similar Questions