Calculate the standard entropy of vaporization of ethanol, C2H5OH, at 285.0 K, given that the molar heat capacity at constant pr
1 answer:
Answer: The standard entropy of vaporization of ethanol is 0.275 J/K
Explanation:
Using Gibbs Helmholtz equation:
For a phase change, the reaction remains in equilibrium, thus
Given: Temperature = 285.0 K
Putting the values in the equation:
Thus the standard entropy of vaporization of ethanol is 0.275 J/K
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Answer:
To prepare 0,2 L of a 0,1M solution of a phosphate buffer to a pH of 7,2 you need to add 1,05 mL of 6M HCl, 2,722 g of K₂HPO₄ and complete 0,2 L with water.
Explanation:
The acid equilibrium of phosphate buffer for a pH of 7,2 is:
H₂PO₄⁻ ⇄ HPO₄²⁻+ H⁺ pka = 6,86
Using Henderson-Hasselbalch formula:
pH = pka + log₁₀
7,2 = 6,86 + log₁₀
2,18776 = <em> (1)</em>
You need to add 0,2L× 0,1M = 0,02 moles of phosphate buffer, that means:
0,02 moles = H₂PO₄⁻ + HPO₄²⁻ <em>(2)</em>
Replacing (2) in (1):
H₂PO₄⁻: <em>6,2739x10⁻³ moles</em>
Thus,
HPO₄²⁻: 0,013726 moles
K₂HPO₄ reacts with HCl thus:
K₂HPO₄ + HCl → KH₂PO₄ + KCl
Thus, you need to add 0,02 moles of K₂HPO₄ that will react with 6,2739x10⁻³ moles of HCl To produce the necessary moles for the buffer:
0,02 moles of K₂HPO₄× = <em>2,722 g</em>
6,2739x10⁻³ moles of HCl÷ 6 M = 1,05x10⁻³ L ≡<em> 1,05 mL of 6M HCl</em>
Thus, to prepare 0,2 L of a 0,1M solution of a phosphate buffer to a pH of 7,2 you need to add 1,05 mL of 6M HCl, 2,722 g of K₂HPO₄ and complete 0,2 L with water.