Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2 O(g) ⇌ 3H2 (
g) + CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4 , 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C?
Let's consider the following reaction at equilibrium.
CH₄(g) + H₂O(g) ⇌ 3 H₂(g) + CO(g)
The concentration equilibrium constant (Kc) is the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.
74.62 g of magnesium oxide is formed from 45.00 g magnesium so 74.62-45.00= 29.62 g of oxygen is consumed or in other words a new compound is formed in the burning of magnesium in oxygen with a heavier mass than the pure magnesium.
<span>Now we add 0.15 mol of naoh to 1.00 liter of the solution that was given in part 1. what is the ph of the solution after the naoh addition? answer in units of ph.
