Consider the equilibrium 2NOCl (g) <---> 2NO (g) + Cl2 (g). In a 1 L container @ equilibrium there are 1.0 mol NOCL, 0.70 mol NO, and 0.40 mol Cl2. @ constant temperature and volume, 0.10 mol NaCl is added. What are the concentrations in the "new" equilibrium in comparison to the concentrations in the "old" equilibrium (are the concentrations of the new equilibrium greater or less than their original concentrations for each).

To determine the concentrations in the "new" equilibrium, we can use the concept of stoichiometry and Le Chatelier's principle. Let's break down the steps:

Step 1: Identify the initial concentrations before adding NaCl.
In the "old" equilibrium, the initial concentrations are:
[NOCl] = 1.0 mol/L
[NO] = 0.70 mol/L
[Cl2] = 0.40 mol/L

Step 2: Determine the effect of adding NaCl.
Since NaCl is not part of the reaction equation, it does not directly affect the equilibrium concentrations of NOCl, NO, or Cl2. Therefore, the concentrations of NOCl, NO, and Cl2 will remain the same.

Step 3: Compare the concentrations in the "new" equilibrium to the concentrations in the "old" equilibrium.
Since adding NaCl does not affect the equilibrium concentrations, the concentrations in the "new" equilibrium will be the same as the concentrations in the "old" equilibrium. Therefore, the concentrations in the "new" equilibrium will be equal to:

[NOCl] = 1.0 mol/L
[NO] = 0.70 mol/L
[Cl2] = 0.40 mol/L

In summary, the concentrations in the "new" equilibrium will be the same as the concentrations in the "old" equilibrium since the addition of NaCl does not impact the equilibrium concentrations of the reactants and products in this particular reaction.