Question

10. (5 pts) Consider the following reaction in equilibrium H2(g) + Br(g) → 2 HBr (g) AH = +68 kJ How will each of the following changes affect the equilibrium concentrations of each chemical: a) addition of HBr(s) b) increasing temperature and timor od moment c) increasing pressure d) decreasing volume of the reacting vessel at constant temperature. e) addition of bromine f) addition of argon neonatology g) addition of catalyst bobb s oods Laboratorio

Answer 1

H2(g) + Brz (3) - 2 HBr (8) OH = +68 kJ Le chatelier's principle A change in any of the factors that determine the equilibrium conditions of system will cause the system to Change in a manner to reduce the affect of the change. Addition of HBr on adding HBr the equilibrium will shift towards left. The concentration of Hz and Bey will increase Increasing Temperature since it is an endothermic reaction on increasing temperature the equilibrium will shift towards right Conc. of Hz and Bre decrease whereas HBr Concentration increases. e Increasing pressure Increasing pressure has no effects on thes egwill It is because the no. of gascous moles of reactant and product are equel. d) decreasing volume It will have no effect on this equilibrium It is because the no. of gaseous moles of reactant and product are equal.

addition of bromine Addition of Bromine will shift the equilibrium towards right. Concentration of Ha decreases whereas HBr Concentration increase. addition of Argon Addition of an inert gas has no effect on the equilibrium reaction. Concentration of all species remain unchanged addition of catalyst Addition of catalyst has no effect on the equilibrium reaction. Concentration of all species remain unchanged.