Equilibrium

Change concentration based solely on changes in total pressure

Decrease concentration of products while increasing concentration of reactants

No effect on either concentration since volume is constant

Increase concentration of both reactants and products equally

Covalent network solid

Metallic Solid

Ionic Solid

Molecular Solid

The shift will favor reactant formation because there are more molecules present initially.

No shift occurs since both sides have gases whose pressures are affected equally by volume changes.

The shift will favor product formation due to fewer moles on that side according to Le Chatelier’s principle.

Pressure changes have no effect on reactions involving solids or liquids only.

Because 'x' is much much less than 'a'

Because 'a' equals zero

Because 'x' equals zero

Because it simplifies calculations without changing results significantly

At least half of the starting material should remain unreacted to ensure a steady supply of ongoing processes.

Both decomposition and synthesis rates must become identical over time, maintaining constant amounts of each substance present.

The system must lose some mass via leakage to secure continuous operation under non-equilibrium conditions.

One reaction needs to reach a point where all the original HCl is decomposed, leaving only the components behind.

PCl5

BF3

CH4

NH3

[Shifts toward side with more moles gas]

['Shifts toward side with fewer moles gas']

['Only affects solids and liquids, so no shift would occur']

['No shift occurs when pressure decreases']

The reaction stops because Q is no longer less than K.

The reaction proceeds in reverse to reach equilibrium, decreasing Q towards K's value.

There is no change in the direction of the reaction; it continues forward until Q equals K.

The equilibrium shifts towards products, increasing Q further from K.

Keq does not change because the catalyst does not alter the position of equilibrium.

Keq increases since the catalyst heightens reaction speed leading to more product formation.

Keq decreases because the catalyst reduces activation energy favoring reactants over products.

Keq remains constant but only until reactant consumption rate equals production rate of products.

Additional NaCl precipitates out until reaching undissolved amount equals original saturation level.

Solution becomes unsaturated temporarily causing quicker dissolution until back at saturation point.

One ions dissociate further increasing Na+ & Cl- concentration until new saturation point reached.

Nothing changes because solids do not affect their own solubility equilibria once saturated.