There are 0.19 ((1.3*3.46)/(0.082*274.27) moles of gas are in the container. This problem can be solved using the ideal gas law formula which stated as PV=nRT where P is the gas' pressure, v is the gas' volume, n is the gas' mole amount, R is the constant gas standard (0.082), and T is the gas' temperature<span>.</span>
Answer:
D. I < III < II
Explanation:
- The osmotic pressure (π) is given by the relation:
<em>π = iMRT.</em>
where, π is the osmotic pressure.
i is van 't Hoff factor.
M is the molarity of the solution.
R is the general gas constant.
T is the temperature.
<em>M, R and T are constant for all solutions.</em>
So, the osmotic pressure depends on the van 't Hoff factor.
- The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved and the concentration of a substance as calculated from its mass.
- For most non-electrolytes dissolved in water, the van 't Hoff factor is essentially 1.
- For most ionic compounds dissolved in water, the van 't Hoff factor is equal to the number of discrete ions in a formula unit of the substance.
For C₂H₆O₂ (non-electrolyte solute): i = 1.
For MgCl₂: i = 3.
It dissociates to give (Mg²⁺ + 2Cl⁻).
For NaCl: i = 2.
It dissociates to give (Na⁺ + Cl⁻).
So, the solute that has the highest osmotic pressure is II. 0.15 M MgCl₂, then III. 0.15 M NaCl, then I. 0.15 M C₂H₆O₂.
<em>D. I < III < II.</em>
<em></em>
The answer is [Pb^2+][Cl-]^2
<span>arsenic is the element often used in rat poison.</span>
