PLEASE HELP Chem

posted by .

Please tell me if these are right.
1.According to Le Chatelier’s principle, what is the effect on the products when N2 is added to the equilibrium mixture of each of the following reactions?

a. 2NH3(g) < = > 3H2(g) + N2(g)
B. N2(g) + O2(g) <= > 2NO(g)
C. 2NO2(g)< => N2(g) +2O2(g)
D. 4NH3(g) + 3O2(g) <= > 2N2(g) +6H2O(g)

A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products

2.Would increasing the volume of the equilibrium mixture of each of the following reactions cause the equilibrium to shift and if so will the shift be toward products or reactants.

a. 2NH3(g) < => 3H2(g) + N2(g)
B. N2(g) +O2(g) <= > 2NO(g)
C. 2NO2(g) <= > N2(g) + 2O2(g)
D. 4NH3(g) +3O2(g) <= > 2N2(g) + 6H2O(g)

A. equilibrium shifts to reactants
B. equilibrium shifts to products
C. equilibrium shifts to reactants
D. equilibrium shifts to products

  • Chem -

    1. correct
    2. reconsider some of the choices, noting that the volume is increased, so decide which side will be favoured by additional volume.

  • PLEASE HELP Chem -

    1.
    A. equilibrium shifts to reactants
    agreed
    B. equilibrium shifts to products
    agreed
    C. equilibrium shifts to reactants
    agreed
    D. equilibrium shifts to products
    Reactants?

    2.
    A. equilibrium shifts to reactants
    No
    B. equilibrium shifts to products
    No
    C. equilibrium shifts to reactants
    No
    D. equilibrium shifts to products
    agreed

    For part 2 if the pressure was increased then the equilibrium shifts in such a way as to oppose the change, i.e. will shift to a smaller volume. As moles are equivalent to volume then you can read these as e.g. equation A
    2 mole => 4 moles. So increasing the pressure will move the equilibrium towards the reactants.
    In the case of incareasing the volume, the pressure must decrease, so the equilibrium will shift in the opposite direction to a pressure increase. That is to a larger total volume, so the equilibria will shift in the direction that has the larger number of moles.
    For equation A
    2 mole => 4 moles. So decreasing the pressure or increasing the volume will move the equilibrium towards the products.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem.....

    Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation: CO(g)+ 2H2(g) <---> CH3OH(g) H = …
  2. chem

    How do these things shift the direction of a chemical reaction?
  3. chemistry

    RE: Le Chatelier's principle. this was the whole question i was given. Write a short account of around 250 words in total, with reference to Le Chatelier’s principle, in which you explain the following: (i) The effect on the equilibrium …
  4. Chem

    Please tell me if these are right. 1.According to Le Chatelier’s principle, what is the effect on the products when N2 is added to the equilibrium mixture of each of the following reactions?
  5. Chemistry - Le Chatelier's principle(help)

    Le Chatelier's principle states that " a dynamic equilibrium tends to respond as to relieve the effect of any change in the conditions that affect the equilibrium." I understand the above, now i am trying to predict the response of …
  6. Chemistry

    According to Le Chatelier's principle, does the equilibrium shift to the products or reactants when O2 is added to the equilibrium mixture of the following: A. 302(g) - 2O3(g)
  7. chemistry

    a. what is the effect on the Kc when the temperature of an exothermic reaction is lowered?
  8. chemistry help plz

    Le chatelier's principle? co(g)+cl2(g)=cocl2(g)is reversible and ,after a certain amount of time ,will reach equilibrium.Explain,using Le chatelier's principle,what effect: 1)increasing the pressure (at constant temperature) 2)increasing
  9. Chemistry

    Given the following exothermic, equilibrium reaction: 3 H2(g) + N2(g) <--> 2NH3(g) Using Le Chatelier's Principle, which of the following changes would shift the equilibrium toward more production of NH3?
  10. chemistry

    consider equilibrium equation below `Mg(NO3)2(aq) + 2Na(OH)(aq) <--> Mg(OH)2(s) + 2NaNO3 (aq) If NH3 is added, according to Le Chatelier's Principle, which way would reaction shift?

More Similar Questions