Question

Hydrogen bromide is farmed by a reaction between hydrogen gas and bromine vapour, according to the following equation
H2(g) + Br2(g) - 2HBr(g) Keq=3.5
calculate the equillibrium concentrations of all gases if .040 moles of H2(g) and 0.60 moles of Br2(g)
are placed in a 4.0L container

Answer 1

Task:

Hydrogen bromide is farmed by a reaction between hydrogen gas and bromine vapour, according to the following equation

$\mathrm{H2(g) + Br2(g) - 2HBr(g)Keq = 3.5}$

calculate the equilibrium concentrations of all gases if 0.40 moles of

$\mathrm{H2(g)}$ and 0.60 moles of $\mathrm{Br2(g)}$

are placed in a 4.0L container

Answer:

$\mathrm{H}_2(\mathrm{g}) + \mathrm{Br}_2(\mathrm{g}) = 2\mathrm{HBr}(\mathrm{g})$

For concentration is used formula $\mathrm{C} = \mathrm{n}(\mathrm{moles}) / \mathrm{V}(\mathrm{L})$

Answer:

$$\mathrm {C} \left(\mathrm {H} _ {2}\right) = 0 \mathrm {M}$$ $$\mathrm {C} \left(\mathrm {B r} _ {2}\right) = 0. 0 5 \mathrm {M}$$ $$\mathrm {C} (\mathrm {H B r}) = 0. 2 \mathrm {M}$$