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

Answer 1

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.