Chemistry

posted by .

For the reaction given, the value of the equilibrium of the constant at 400 K is 7.0. Br2(g)+ Cl2(g)=2BrCl(g)
Does the:
Reaction proceed to the left?
Reaction proceed to the right?
Partial pressure represent a system in an equation?

  • Chemistry -

    Write the K expression. Now, to have K 7.0 (greater than 1.0), must products or reactants be greater or less?

  • Chemistry -

    The reaction is favoring the products. In other words when you have a reaction whose number is 0 you are at a perfect equilibrium, when you have some number smaller than that you have a greater number of reactants than products. When you are above that you a greater number of products than compared to reactants. How do I know this? Kc= products/reactants

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    The equilibrium constant for the reaction of bromine and chlorine to form bromine chloride under certain conditions is 4.7x10-2. Cl2(g) + Br2(g) --> 2BrCl(g) K= 4.7 x 10-2 What is the equilibrium constant for the following reaction …
  2. chemistry

    Choose all of the following statements about the equilibrium constant K that are true: (a) If the K value for a reaction is > 1 then Go must be negative for this reaction (b) A large value for K implies there is a strong driver …
  3. Chemistry

    The initial pressure for the compounds involved in the reaction shown were determined to be P(Br2(g)) = 0.5417 atm, P(Cl2(g)) = 0.6962 atm, P(BrCl(g)) = 0.3442 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if …
  4. chemistry

    On this problem I keep getting the wrong answer. I am subtracting the initial concentration of Cl2 by the equilibrium concentration then using the difference to subtract for the rest using the mole ratios. Then i used the keq constant …
  5. Chemistry

    In which direction will the net reaction proceed. X(g) + Y(g) <==> Z(g) .. Kp = 1.00 at 300k for each of these sets of initial conditions?
  6. Chemistry

    The Kc for the following reaction at 940oC is 1.38. Given the concentrations [CO2] = 0.500 M, [H2] = 0.425 M, [CO] = 0.610 M and [H2O] = 0.695 M, one can conclude that: H2(g) + CO2(g) ↔ CO(g) + H2O(g) Question 8 options: A) the …
  7. Chemistory

    The reaction has an equilibrium constant of = 0.154. If 6.60 of , 4.30 of , and 11.60 of are added to a reaction vessel with a volume of 5.30 , what net reaction will occur?
  8. Chemistry

    If the initial concentration of BrCl(g) is 4.680 mol/L, calculate the % of BrCl(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kc at 500.0 K is 32.00. The initial concentration …
  9. Equilibrium

    The following reaction has an equilibrium constant (Keq) of 160. 2 NO2(g) <--> 2 NO(g) + O2(g) What will be the reaction quotient (Q) and in which direction will the reaction proceed if the partial pressure of NO2 is 5.0*10^-4 …
  10. science

    When Q < K, what can you conclude about the reaction?

More Similar Questions