Yes, in that case it still applies. If reactants ar given and zero produccts are given common sense tells you that it MUST go the right and the reactant(s) lose and the product(s) gain.
The second possibility is that you have zero reactants but you start with the product. In that case common sense tells you it MUST go to the left and form reactants at the expense of the product(s).
The third case involves say you have a reaction like
2A + B ==> C and values are given for A and C or even A, B and C. Then common sense doesn't help much. What you do in that case is set up Qc, plug in the numbers and see if Qc is <, =, or > Kc.
If Qc<Kc the equilibrium point is to the right(more products and fewer reactants). If Qc > Kc, the reverse. If Qc = Kc the reaction is at equilibrium.
When doing an ICE Chart in Chemistry, when do you know whether the C is a negative or positive?
I was told if the problem gives us reactant concentrations and no product concentration then the reaction goes forward and make the reactant lose and the product gain for example I2 (g) + H2 (g) ----> 2HI
However, what if it's 2BrCl -----> Br2 + Cl2 , would it still apply?
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