In which of the following reactions would increasing pressure at constant temperature change the concentrations of reactants and products, based on le châteliers principle? (a) n2 (g) + 3h2 (g) ↔ 2nh3 (g) (b) n2o4 (g) ↔ 2no2 (g) (c) n2 (g) + 2o2 (g) ↔ 2no2 (g) (d) 2n2 (g) + o2 (g) ↔ 2n2o (g) (e) all of the above

E) all of the above

Explanation:

The pressure is a measure of the force of the gases, so when the number of moles of gases increases, the pressure also increases (in an isothermic process). By the principle of Le Chatelier, if the pressure increases, the equilibrium must be dislocated to form the fewer moles of gases compounds.

So, the increase in pressure only will not affect the concentrations of the reactants if there are no gases compounds, or if there is the same number of moles gases in reactants and products. So, in all of the reactions, a change in the temperature will change the equilibrium.

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

its first and third is your answer i did the qustion the fourth isnt right