Monday
April 21, 2014

Homework Help: chem

Posted by Tracy on Monday, November 19, 2012 at 12:26pm.

a.) At equilibrium, the molar concentrations for reactants and products are found to be [I2] = 0.50 M,[Cl2] = 0.60 M, and [ICl] = 5.0 M. What is the equilibrium constant (Kc) for this reaction?
b.) The concentration of I2 is increased to 1.5 M, disrupting equilibrium. Calculate the new ratio of products to reactants with this higher concentration of iodine. Assume that the reaction has not yet regained equilibrium.
the reaction is I2 + Cl2 = 2ICl pls help

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chem - Given the concentrations, calculate the equilibrium constant for this ...
chemistry - balance:H2(g)+S2(g)------->H2S(G)+heat A.) how would the ...
chem - The molar concentrations for the reactants and products at equilibrium ...
Chemistry - Consider the equilibrium 2NOCl (g) <---> 2NO (g) + Cl2 (g). In...
chemistry(please check) - Just made it a new post didnt what it to get ...
Chem - 4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all ...
Chem - 4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all ...
Chem - 4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all ...
Chemistry(Please check, thank you!) - I completed a lab to find the ...
Chemistry(Urgent, please check) - I completed a lab to find the determination ...

Search
Members