Posted a question earlier but it was the wrong question. If anyone could help it would great if you could explain this would help also.
Thanks
^ = subscript
Calculate ke for(equlibrium concentration below problem
2CO^2(g) + heat 2CO(g) + O^2
[0.103] [0.024] [1.18 x 10^2]
1. You have no arrow. How do we separate the reactants from the products? I assume it is
2CO2 + heat ==> 2CO + O2
2. You don't need to write ^ for subscripts. The ^ sign is reserved for exponents and on these boards it is understood that we can't write subscripts; therefore, NO2 means NO2. 10^-3 means 10-3.
3. What is the Ke expression? Isn't it
(CO)^2(O2)/(CO2)^2
4. If that second line you have denotes equilibrium concentrations, just plug into the appropriate boxes in the Ke expression (written in 3 above) and calculate.
Not sure, sorry.
To calculate the equilibrium constant (Ke) for this given chemical equation, we need to use the equilibrium concentrations of the reactants and products. In this case, the equation is:
2CO2(g) + heat --> 2CO(g) + O2(g)
The equilibrium concentrations are given as:
[CO2] = 0.103 M
[CO] = 0.024 M
[O2] = 1.18 × 10^2 M
The equilibrium constant (Ke) is calculated using the molar concentrations of the products divided by the molar concentrations of the reactants, each raised to the power of their respective stoichiometric coefficients. In this case, the stoichiometric coefficients are 2 for CO2 and CO, and 1 for O2.
The formula for Ke is:
Ke = ([CO]^2 × [O2]) / ([CO2]^2)
Substituting the given values into the equation, we get:
Ke = (0.024^2 × 1.18 × 10^2) / (0.103^2)
To find the solution, we can plug these values into a calculator or computer software to obtain the numerical value for Ke.