How will the osmotic pressure of an aqueous solution change as evaporation occurs?

When evaporation occurs, the osmotic pressure increases.

Explanation:

Osmotic pressure is defined as the minimum excess pressure that can be applied on the solution to prevent the entry of the solvent into the solution through a semipermeable membrane. The formula to calculate osmotic pressure is given by the equation:

where,

= osmotic pressure

c = concentration of solute

R = gas constant

T = temperature

As, concentration of solute is directly proportional to the osmotic pressure. So, when concentration increases, osmotic pressure also increases and vice-versa.

Evaporation is a process when liquid changes its state to gaseous state by increasing the temperature. In this process, solvent particles escape and more and more solute particles remain in the solution. So, concentration of solute particles increases.

Hence, evaporation causes increase in the osmotic pressure.

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.