I am given the equation: H2(g) + F2(g) is in equilibrium with 2HF(g)
Here is the question: Assume that the reaction for the formation of gaseous hdrogen fluoride from hydrogen gas and fluorine gas has an equilibrium constant of 1.15 X 10^2 at a certain temperature. In a particular experiment, 1.000 mol of H2(g) and 2.500 mol F2(g) were added to a 3.00L container. Calculate the equilibrium concentrations of all species.
So, I figured out that the initial for the H2 and the F2 are 3.3 x 10^-1 and 8.3 x 10^-1 respectively. For now, the initial of 2HF is 0. I am correct so far. I am already given the equilibrium constant for 2HF, which is 1.15 x 10^2. That means I take its initial (0) and add 1.15 x 10^2 to figure out its change. I take that same change for the other initials, but I subtracted and halved them. When I calculated their equilibriums, however, I got the wrong answer. Where did I go wrong and how do I correct it?
Here is the question: Assume that the reaction for the formation of gaseous hdrogen fluoride from hydrogen gas and fluorine gas has an equilibrium constant of 1.15 X 10^2 at a certain temperature. In a particular experiment, 1.000 mol of H2(g) and 2.500 mol F2(g) were added to a 3.00L container. Calculate the equilibrium concentrations of all species.
So, I figured out that the initial for the H2 and the F2 are 3.3 x 10^-1 and 8.3 x 10^-1 respectively. For now, the initial of 2HF is 0. I am correct so far. I am already given the equilibrium constant for 2HF, which is 1.15 x 10^2. That means I take its initial (0) and add 1.15 x 10^2 to figure out its change. I take that same change for the other initials, but I subtracted and halved them. When I calculated their equilibriums, however, I got the wrong answer. Where did I go wrong and how do I correct it?