Write equilibrium constant expressions for K, and Kp for the
formation of nickel tetracarbonyl, which is used to separate nickel from other
impurities:
Ni(s) + 4C0(g) -> Ni(CO), (g)
C'mon. You really need to know how to do this yourself. Here's how you do ALL of them. Kc. Multiply concentrations of the products and divide by the concentraton of the reactants. Then raise EACH product or reactant to a power which is the coefficient in the balanced equation. If it's Kp you want instead of concentrations use partial pressure. For Kc for example:
A + B ==> 2C + 3D
Kc = (C)^2*(D)^3/(A)*(B) or
Kp = pC^2*pD^3/pA*pB OR if you have Kc and want to convert to Kp that can be done this way.
Kp = Kc*(RT)^delta n where delta n = mols procuts-mols reactants. In the case of the equation above that will be (2+3) = (1+1) = 3
Post any follow up questions here and tell me what trouble you're having. This is basic and you need to understand it completely in order to understand what's coming.
oops. typos. See bold/italics where corrected.
Kp = Kc*(RT)^delta n where delta n = mols products - mols reactants. In the case of the equation above that will be (2+3) - (1+1) = 3.
The equilibrium constant expression for K is given by:
K = [Ni(CO)4(g)] / [Ni(s)] * [CO(g)]^4
Where [Ni(CO)4(g)] represents the concentration of nickel tetracarbonyl gas, [Ni(s)] represents the concentration of solid nickel, and [CO(g)] represents the concentration of carbon monoxide gas.
The equilibrium constant expression for Kp is similar but takes into account the partial pressures instead of concentrations:
Kp = P(Ni(CO)4(g)) / P(Ni(s)) * (P(CO(g)))^4
Where P(Ni(CO)4(g)) represents the partial pressure of nickel tetracarbonyl gas, P(Ni(s)) represents the partial pressure of solid nickel, and P(CO(g)) represents the partial pressure of carbon monoxide gas.
To write the equilibrium constant expressions for a reaction, we first need to write the balanced chemical equation:
Ni(s) + 4CO(g) -> Ni(CO)4(g)
The equilibrium constant expression, K, is defined as the ratio of the concentrations (or partial pressures in the case of gases) of the products to the concentrations (or partial pressures) of the reactants at equilibrium.
For K, we express the concentrations of the products and reactants using their respective molar amounts at equilibrium:
K = [Ni(CO)4(g)] / [Ni(s)] * [CO(g)]^4
Here, [Ni(CO)4(g)] represents the equilibrium concentration of nickel tetracarbonyl, [Ni(s)] represents the equilibrium concentration of nickel (solid), and [CO(g)] represents the equilibrium concentration of carbon monoxide.
In the case of Kp, which is the equilibrium constant expressed in terms of partial pressures for gaseous species, we use the ideal gas law. Since nickel and carbon monoxide are both gases, we can express their partial pressures instead of their concentrations:
Kp = (P(Ni(CO)4(g)) / (P(Ni(s))) * (P(CO(g)))^4
Here, P(Ni(CO)4(g)) represents the partial pressure of nickel tetracarbonyl, P(Ni(s)) represents the partial pressure of nickel, and P(CO(g)) represents the partial pressure of carbon monoxide.