Adsorption is the process by which atoms, ions, or molecules from a gas, liquid, or dissolved solid adhere to a surface.

'A' is the frequency factor in the Arrhenius equation, which represents the number of collisions that result in a reaction.

'R' in the ideal gas equation PV = nRT represents the universal gas constant, which relates the energy scale to the temperature scale.

Absolute zero is defined as 0 Kelvin, the theoretical temperature at which a system's entropy reaches its minimum value.

In the ideal gas equation, R is the universal gas constant, which relates the pressure, volume, temperature, and number of moles of a gas.

Activation energy is the minimum energy required for reactants to collide and form products, initiating the reaction.

Increasing the concentration of B will shift the equilibrium to the left, decreasing the concentration of A.

Increasing the volume decreases the pressure, and according to Le Chatelier's Principle, the equilibrium will shift to the right to favor the formation of more gas molecules (C).

Decreasing the concentration of SO3 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's Principle.

Increasing the concentration of O2 will shift the equilibrium to the right, favoring the production of SO3.

Adding SO3 will shift the equilibrium to the left to favor the formation of reactants, according to Le Chatelier's Principle.

Increasing the pressure will shift the equilibrium to the right, favoring the formation of SO3, as it has fewer moles of gas (2 moles) compared to the reactants (3 moles).

Increasing the volume decreases the pressure, and the equilibrium will shift to the side with more moles of gas to counteract the change.

Removing A will shift the equilibrium to the left to produce more A, according to Le Chatelier's Principle.

Increasing pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas.

Adding more CO increases its concentration, which shifts the equilibrium to the right to produce more CH3OH.

Increasing the pressure favors the side with fewer moles of gas. In this case, the right side has fewer moles (1 mole of CH3OH) compared to the left (3 moles), so the equilibrium shifts to the right.

If the reaction is exothermic, decreasing the temperature will shift the equilibrium to the right to produce more products (CH3OH).

Increasing the concentration of HI will shift the equilibrium to the left to reduce the concentration of HI, according to Le Chatelier's Principle.

According to Le Chatelier's principle, increasing the concentration of a product (NH3) will shift the equilibrium to the left, decreasing N2.

Decreasing the concentration of NH3 will shift the equilibrium to the right to produce more NH3, according to Le Chatelier's Principle.

Removing Cl2 decreases its concentration, causing the equilibrium to shift to the right to produce more Cl2.

'a' accounts for the attractive forces between particles, while 'b' accounts for the volume occupied by the gas particles in the van der Waals equation.

BF3 has a trigonal planar geometry with bond angles of approximately 120°.

CH4 has a tetrahedral geometry with bond angles of approximately 109.5 degrees.

In CH4, the carbon atom has four bonding pairs and no lone pairs, leading to sp3 hybridization.

Hydrogen bonding occurs in H2O due to the presence of highly electronegative oxygen atoms bonded to hydrogen, creating strong dipole interactions.

C2 has a triple bond between the two carbon atoms, resulting in the shortest bond length compared to the others.

C2H4 has a double bond between the carbon atoms, indicating sp2 hybridization.

SiCl4 has four bonding pairs and no lone pairs, leading to sp3 hybridization of the silicon atom.