A test reaction is done starting with only methane and excess water in the autoclave. If the initial concentration of methane is 0.110 mol/L, and the methane concentration at equilibrium is 0.010 mol / L, then the equilibrium concentration of hydrogen is _________ mol / L
In the given test reaction, methane (CH4) reacts with water (H2O) to form hydrogen gas (H2) and carbon dioxide (CO2) according to the following balanced equation:
CH4 + 2H2O -> CO2 + 4H2
From the equation, we can see that 1 mole of methane (CH4) produces 4 moles of hydrogen (H2) at equilibrium. Therefore, the change in hydrogen concentration is 4 times the change in methane concentration.
The change in methane concentration is calculated by subtracting the equilibrium concentration from the initial concentration:
Change in methane concentration = 0.110 mol/L - 0.010 mol/L = 0.100 mol/L
Since the change in hydrogen concentration is 4 times the change in methane concentration, the change in hydrogen concentration is:
Change in hydrogen concentration = 4 * 0.100 mol/L = 0.400 mol/L
Therefore, the equilibrium concentration of hydrogen is 0.400 mol/L.