Calculate the enthalpy change, ΔH, for the process in which 31.6 g of water is converted from liquid at 3.2 ∘C to vapor at 25.0°
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Complete Question
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Answer:
The value is
Explanation:
From the question we are told that
The voltage of the cell is
Generally is mathematically represented as
Where is the equilibrium constant for this auto-ionization of water with a value
Generally the is mathematically represented as
=>
=>
This is mathematically represented as
Where n is the number of moles which in this question is n = 1
So
=>
So
=>
=>
Molarity of concentrated nitric acid = 15.9 M
Volume of the stock solution to be prepared = 500.0 mL
Concentration of the stock that is to be prepared = 0.750 M
Calculating moles from molarity and volume of stock:
Calculating volume of concentrated nitric acid to be taken for the preparation of stock solution:
Converting L to mL:
= 23.6 mL
Volume of distilled water to be added to 23.6 mL of 15.9 M nitric acid to get the given concentration = 5000.0mL-23.6mL=976.4 mL
Therefore, 976.4 mL distilled water is to be added to 23.6 mL of 15.9 M nitric acid solution to prepare 500.0 mL of 0.750M nitric acid.