If you make a solution by dissolving 1.0 mol of fecl3 into 1.0 kg of water, how would the osmotic pressure of this solution compare with the osmotic pressure of a solution that is made from 1.0 mol of glucose in 1.0 kg of water? one-half as large the same twice as large four times as large

Given the solutions are 1.0 mol of in 1.0 kg water and 1.0 mol glucose in 1.0 kg water.

Osmotic pressure of a solution can be calculated using the formula:

Osmotic pressure, π = iMRT

Where i is the number of ions the solute can give in solution.

M is the molar concentration.

R is gas constant.

T is the temperature in Kelvin scale.

When we compare both the solutions, all the other variables that the osmotic pressure are same except the i value.

For solution i = 4  as it can give 4 ions in solution, 1 and 3 ions.

Glucose is a non electrolyte, therefore it cannot give any ions in solution. So, for glucose solution i = 1

Hence, we can conclude that the osmotic pressure of solution will be 4 times that of glucose solution of same concentration.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.