Answer:
- m = 1,000/58.5
- b = - 1,000 / 58.5
1) Variables
- molarity: M
- density of the solution: d
- moles of NaCl: n₁
- mass of NaCl: m₁
- molar mass of NaCl: MM₁
- total volume in liters: Vt
- Volume of water in mililiters: V₂
- mass of water: m₂
2) Density of the solution: mass in grams / volume in mililiters
3) Mass of NaCl: m₁
Number of moles = mass in grams / molar mass
⇒ mass in grams = number of moles × molar mass
m₁ = n₁ × MM₁
4) Number of moles of NaCl: n₁
Molarity = number of moles / Volume of solution in liters
M = n₁ / Vt
⇒ n₁ = M × Vt
5) Substitue in the equation of m₁:
m₁ = M × Vt × MM₁
6) Substitute in the equation of density:
d = [M × Vt × MM₁ + m₂] / (1000Vt)
7) Simplify and solve for M
- d = M × Vt × MM₁ / (1000Vt) + m₂/ (1000Vt)
- d = M × MM₁ / (1000) + m₂/ (1000Vt)
Making the simplistic assumption that the dissolved NaCl(s) does not affect the volume of the solvent water means 1000Vt = V₂
- d = M × MM₁ / (1000) + m₂/ V₂
m₂/ V₂ is the density of water: 1.00 g/mL
- d = M × MM₁ / (1000) + 1.00 g/mL
- M × MM₁ / (1000) = d - 1.00 g/mL
- M = [1,000/MM₁] d - 1,000/ MM₁
8) Substituting MM₁ = 58.5 g/mol
- M = [1,000/58.5] d - [1,000/ 58.5]
Comparing with the equation Molarity = m×density + b, you obtain:
- m = 1,000/58.5
- b = - 1,000/58.5
is the ΔS°rxn for the formation of Cu₂O(s) from its elements.
WHAT IS ΔS°rxn FOR THE REACTION ?
The direction of spontaneous change is the direction in which total entropy increases. Total entropy change, also called the entropy change of the universe, is the sum of the entropy change of a system and of its surroundings
Standard entropy change of below reaction (ΔS°
)
∴ ΔH° = - 168.6 KJ/mol
Now, 
![= S^o_{Cu_2 O(s)} - [2 * S^o_{Cu(s)} + \frac{1}{2}(S^o_{O_2(g)}]](https://tex.z-dn.net/?f=%3D%20S%5Eo_%7BCu_2%20O%28s%29%7D%20-%20%5B2%20%2A%20S%5Eo_%7BCu%28s%29%7D%20%2B%20%5Cfrac%7B1%7D%7B2%7D%28S%5Eo_%7BO_2%28g%29%7D%5D)
![= (93.1 J/molK)- [2 * 133.1 + \frac{1}{2}(205.0)]J/molK](https://tex.z-dn.net/?f=%3D%20%2893.1%20J%2FmolK%29-%20%5B2%20%2A%20133.1%20%2B%20%5Cfrac%7B1%7D%7B2%7D%28205.0%29%5DJ%2FmolK)
Thus, -75.6 J/mol K is the ΔS°rxn for the formation.
Learn more about ΔS°rxn FOR THE REACTION are:
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