Consider the following system at equilibrium at 573 k: 2nocl(g) + 18.4 kcal2no(g) + cl2(g) if the temperature on the equilibrium system is suddenly increased: the reaction must: a. run in the forward direction to restablish equilibrium. b. run in the reverse direction to restablish equilibrium. c. remain the same. already at equilibrium. the concentration of cl2 will: a. increase. b. decrease. c. remain the same.

After increasing the temperature of the system:

The reaction must: Run in the forward direction to restablish equilibrium.

Already at equilibrium. The concentration of Cl2 will: Increase.

Explanation:

The equilibrium constant, for an endothermic reaction (ΔH ° positive), increases with increasing temperature.

The principle of Le Châtelier indicates that if an equilibrium mixture is heated, and consequently its temperature increases, there will be a net reaction in the direction that counteracts the disturbance caused by the increase in temperature. For an endothermic reaction, the direct reaction absorbs energy in the form of heat.

Consequently, the equilibrium shifts to the side of the products, which means that Kc increases with increasing temperature.

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.