At 1200 K a gaseous mixture contains 0.30 moles of carbon monoxide, 0.10 moles of hydrogen, 0.20 moles of water vapor and 0.059 moles of methane in a 1.00 liter container. Determine whether or not equilibrium has been reached for the following reaction:
CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g)
For the questions that you posted, can you please also post any work that you have done, or let us know specifically where you are getting stuck? Thanks!
To determine whether equilibrium has been reached for the given reaction, we need to compare the concentrations of the reactants and products with respect to their stoichiometric coefficients.
First, we need to calculate the concentrations of each species in the mixture. Concentration can be calculated by dividing the number of moles of a species by the volume of the container.
Concentration of CO = 0.3 moles / 1.0 L = 0.3 M
Concentration of H2 = 0.1 moles / 1.0 L = 0.1 M
Concentration of CH4 = 0.059 moles / 1.0 L = 0.059 M
Concentration of H2O = 0.2 moles / 1.0 L = 0.2 M
Now, let's compare the concentrations of the reactants and products according to their stoichiometric coefficients.
Coefficients:
CO(g) --> 1
H2(g) --> 3
CH4(g) --> 1
H2O(g) --> 1
According to the balanced equation, for every 1 mole of CO(g) reacting, we should have 3 moles of H2(g) and 1 mole each of CH4(g) and H2O(g) being produced.
Comparing the concentrations, we can see that the concentration of CO is higher than the concentrations of CH4 and H2O. However, the concentration of H2 is lower than the concentrations of CH4 and H2O.
Based on this comparison, we can conclude that equilibrium has not been reached for the reaction. Equilibrium would be reached when the concentrations of the reactants and products are in accordance with their stoichiometric coefficients.