Consider the following system at equilibrium at 298 K: 2 NOBr (g) + 3.85 kcal 2
ID: 635248 • Letter: C
Question
Consider the following system at equilibrium at 298 K: 2 NOBr (g) + 3.85 kcal 2 NO (g) + Br2 (g) Indicate whether each individual change would favor the production of NO (g). Evaluate each change separately, assuming that all other conditions remain constant. ANSWER YES OR NO
Decreasing the temperature. yes or no
Decreasing the pressure. yes or no
Decreasing the volume. yes or no
Removing NOBr . yes or no
Adding Br2 . yes or no
____________________________
Consider the following system at equilibrium at 648 K:
SO2Cl2 (g) + 16.1 kcal SO2 (g) + Cl2 (g)
Indicate whether each individual change would favor the production of SO2 (g). Evaluate each change separately, assuming that all other conditions remain constant.
Decreasing the temperature.
_____yes no
Decreasing the pressure.
_____yesno
Decreasing the volume.
_____yes no
Removing SO2Cl2 .
_____yes no
Adding Cl2 . ________ YES NO
Decreasing the temperature.
_____yes no
Decreasing the pressure.
_____yesno
Decreasing the volume.
_____yes no
Removing SO2Cl2 .
_____yes no
Adding Cl2 . ________ YES NO
Explanation / Answer
Ans 1
The given equillibrium reaction
2 NOBr (g) + 3.85 kcal = 2 NO (g) + Br2 (g)
Heat is added into the system
The reaction is endothermic
Mole of reactants < moles of products
From the Le Chatelier's principle
For the production of NO (g)
Decreasing the temperature - no
The reaction is endothermic so heat is required to maintain the temperature of the reaction so that the products formation take place.
Decreasing the pressure. yes
Mole of reactants < moles of products
pressure decreases due to an increase in volume, because products have more moles, so more NO will produce
Decreasing the volume. no
Mole of reactants < moles of products
increase in volume, because products have more moles, so more NO will produce
Removing NOBr . no
More NOBr will produce.
Adding Br2 . no
More NOBr will produce.