The molecular mass of is:
2·1 + 1·32 + 4·16 = 98 g/mol
The amount of solute, expressed by mol, is:
The molar concentration definition is:
Doing the calculations:
(If you detect any mistakes in my English report me them, please).
Answer:
Boiling point for the solution is 100.237°C
Explanation:
We must apply colligative property of boiling point elevation
T° boiling solution - T° boiling pure solvent = Kb . m
m = molalilty (a given data)
Kb = Ebulloscopic constant (a given data)
We know that water boils at 100°C so let's replace the information in the formula.
T° boiling solution - 100°C = 0.512 °C/m . 0.464 m
T° boiliing solution = 0.512 °C/m . 0.464 m + 100°C → 100.237 °C
The volume of 1.50 moles of (Cl2) gas at STP is 33.6 (L/m)
Adding energy can put the reaction in a state of equilibrium because more energy allows the reverse reaction, which is endothermic, to occur along with the forward reaction
Hope this helps