1. Write the equilibrium expressions for the following reactions:
a) 2 N2O(g) + O2(g) 4 NO(g)
b) H2(g) + CO2(g) H2O(g) + CO(g)
c) 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g)
d) 3 H2(g) + N2(g) 2 NH3(g)
e) H2(g) + Cl2(g) 2HCl(g)
f) 2 SO2(g) + O2(g) 2 SO3(g)
Im not asking to do all my hw
I just want to know what do
How do you multiple O2 to ^2
Is it with the mass or ?
To write the equilibrium expressions for the given reactions, we need to express the concentrations of the reactants and products in terms of their molarities and include the corresponding stoichiometric coefficients as exponents. The equilibrium constant (K) is then calculated as the ratio of the product concentrations to the reactant concentrations, each raised to the power of their respective stoichiometric coefficients.
For the given reactions:
a) 2 N2O(g) + O2(g) ⇌ 4 NO(g)
The equilibrium expression is: K = [NO]^4 / [N2O]^2 * [O2]
b) H2(g) + CO2(g) ⇌ H2O(g) + CO(g)
The equilibrium expression is: K = [H2O] * [CO] / [H2] * [CO2]
c) 4 HCl(g) + O2(g) ⇌ 2 Cl2(g) + 2 H2O(g)
The equilibrium expression is: K = [Cl2]^2 * [H2O]^2 / [HCl]^4 * [O2]
d) 3 H2(g) + N2(g) ⇌ 2 NH3(g)
The equilibrium expression is: K = [NH3]^2 / [H2]^3 * [N2]
e) H2(g) + Cl2(g) ⇌ 2 HCl(g)
The equilibrium expression is: K = [HCl]^2 / [H2] * [Cl2]
f) 2 SO2(g) + O2(g) ⇌ 2 SO3(g)
The equilibrium expression is: K = [SO3]^2 / [SO2]^2 * [O2]
By writing the equilibrium expressions, we can quantify the relative amounts of products and reactants at equilibrium using the equilibrium constant, which is specific to each reaction.
Why do I want to do all of your home work? What don't you understand about this? It's products divided by reactants with coefficients for each material becoming the exponent for that material.
For example, f is
K = (SO3)^2/(SO2)^2(O2)