Consider the equilibrium
H₂(g) + Br₂(g) 2HBr(g)
To a 20.0 L flask are added 0.100 moles of H₂ and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br₂ in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

Question

Consider the equilibrium
H₂(g) + Br₂(g) Consider the equilibrium H2(g) + Br2(g) 2HBr(g) To a 20.0 L flask are added 0.100 moles of H2 and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br2 in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

Consider the equilibrium H<sub>2</sub>(g) + Br<sub>2</sub>(g) 2HBr(g) To a 20.0 L flask are added 0.100 moles of H<sub>2</sub> and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br<sub>2</sub> in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

2HBr(g)
To a 20.0 L flask are added 0.100 moles of H₂ and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br₂ in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

Quizplus · Accepted Answer

The Answer of Consider the equilibrium H₂(g) + Br₂(g) 2HBr(g) To a 20.0 L flask are added 0.100 moles of H₂ and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br₂ in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.

Consider the Equilibrium H2(g) + Br2(g) 2HBr(g)

Consider the Equilibrium H₂(g) + Br₂(g) 2HBr(g)