Question

Pressure can be used only for gaseous reactants?
Does it mean all the reactants have to be gaseous?

Answer 1

@Photon336

Answer 2

For example,
C(s) + O2 --> CO2 (g)
Can pressure affect this heterogeneous reaction or do all the reactants need to be gaseous?

Answer 3

\[C(s) + O_{2}(g) -> CO_{2}(g) \]

Answer 4

Yes, as we know we have two words in chemistry. Total pressure of the system or partial pressure of a gas.

Answer 5

well for a gaseous reaction it depends on the partial pressure exerted by each gas

Answer 6

couple of things here to explain

Answer 7

the first is that whenever you have a container of gases

the pressure exerted by each individual gas will be proportional to the mole fraction of that gas.

say you have 1 mole of A and 2 moles of B both gases

first we find out how many total moles of gas we have that's 1+2 = 3 moles of gas.

A + 2B --> AB_{2} and the pressure is 1 atm

\[Gas_{A} \frac{ 1 }{ 2 }*1atm + Gas_{B}\frac{ 2 }{ 3 }*1atm = total pressure \]

Answer 8

Now second point

Answer 9

do you know what the equilibrium constant expression is?

Answer 10

wel, \[\frac{ [C]^{a}[D]^{b}}{ [A]^{c}[B]^{d} } = K_{p}\]

Answer 11

Actually my teacher have not started that yet. She taught my calss kinetic reactions and kinetic energy

Answer 12

what this expression tells us is that we take the concentration of something mol/L for each reactant and raise it to the power of the stoichiometric coefficient that means the number in front of our reactants and products in your balanced reaction.

now this is what i believe you need to know: the fact here is that solids and pure liquids aren't included in this expression, because their concentrations don't change very much over time. So gases will always be included in this expression, and I guess maybe some aqueous solutions too.

so for our reaction