0.75 mol of N₂ and 1.20 mol of H₂ are placed in a 3.0 liter container.When the reaction
N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) reaches equilibrium,[H₂] = 0.100 M.Which of the following is true?

Question

0.75 mol of N₂ and 1.20 mol of H₂ are placed in a 3.0 liter container.When the reaction N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g)reaches equilibrium,[H₂] = 0.100 M.Which of the following is true?

Quizplus · Accepted Answer

We can use the equilibrium constant expression to solve for the concentration of [NH₃]. K_eq = ([NH₃]^2) / ([N₂] * [H₂]^3) We can substitute the given values: K_eq = ((2x)^2) / ((0.75-x) * (0.1)^3) where x is the change in concentration of [N₂] at equilibrium. We can then solve for x: K_eq * ((0.75-x) * (0.1)^3) = (2x)^2 x = 0.2 Therefore, [NH₃] = 2x = 0.4 M. So, the correct choice is B.

075 Mol of N2 and 1

075 Mol of N₂ and 1