Equilibrium

The equilibrium shifts towards the side with fewer gas molecules.

All gases escape from the system, so there is no longer an equilibrium.

Nothing, the volume change has no effect on equilibrium positions.

The equilibrium shifts towards the side with more gas molecules.

It would favor decomposition of hydrogen iodide into hydrogen and iodine gases.

It would shift towards producing more hydrogen iodide due to fewer moles of gas on that side of the equation.

Increased pressure has no effect since all components are gases with similar molar volumes.

It would result in decreased production of hydrogen iodide because it has higher molar mass than reactants.

Causes an immediate shift towards the products.

No effect on the state of equilibrium.

Decreases the equilibrium constant value.

Increases the equilibrium constant value.

The equilibrium shifts toward reactants.

No shift in equilibrium occurs because it's already at balance.

Equilibrium constants become smaller.

The system consumes energy from surroundings faster.

$(a+b)/(c+d)$

$a[A] + b[B]/c[C] + d[D]$

$c[C] + d[D] - a[A] - b[B]$

$[C]^c[D]^d/[A]^a[B]^b$

The position of equilibrium does not change since solid addition doesn't alter gaseous concentrations.

Equilibrium moves towards decomposition producing more gaseous species that counteract increasing total pressure.

It leads directly to production of more solids lowering vapor pressure above solution.

Equilibrium shifts towards NH4Cl formation reducing both NH3(g) and HCl(g).

Shifts left, reducing production of COCl_2.

No change no matter of pressure.

Shifts right, favoring production of COCl_2.

The system will shift toward reactants.

The system will remain at equilibrium without any shift.

The system will produce even more products.

The volume of the container will increase automatically.

The reaction will not proceed.

The reactants are favored.

The products are favored.

The system is at equilibrium.

Q = 2.5, so the reaction shifts right.

Q = 0.25, so the system is already at equilibrium.

Q = 2.5, so the reaction shifts left.

Q = 250, so the reaction shifts right.