A reaction has an equilibrium constant of 8.1×103 at 298 k. at 714 k , the equilibrium constant is 0.74. find δhorxn for the rea
1 answer:
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Answer:
206 mL
Explanation:
In the annexed picture you can see your same question, just in another format.
First we <u>calculate the total moles of CuF₂ that are required in the working solution</u>:
1967 μM ⇒ 1967 / 10⁶ = 1.967 x10⁻³M
1.967 x10⁻³M * 0.275 L = 5.409x10⁻⁴ mol
Now we divide those moles by the concentration of the stock solution, to <u>calculate the volume</u>:
5.409x10⁻⁴ mol ⇒ 5.409x10⁻⁴ * 1000 = 0.5409 mmol
0.5409 mmol ÷ (2.63 mmol/L) = 0.206 L
0.206 L ⇒ 0.206 * 1000 = 206 mL
