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Katarina [22]
3 years ago
5

Which choice is not true of a liquid in a glass capillary with a convex meniscus?

Chemistry
2 answers:
GalinKa [24]3 years ago
6 0
It's false that the liquid has strong cohesive forces (since cohesive forces mean the liquid is essentially attracted to itself, and that would result in a concave meniscus).
Mamont248 [21]3 years ago
5 0
I believe <span>The liquid has strong cohesive forces.</span>
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3 years ago
Freon-12 CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed
LekaFEV [45]

Answer:

percent yield = 40.6 %

Explanation:

The question asks to determine the percent yield, which can be defined as:

percent yield = \frac{actual yield}{theoretical yield} *100

where the actual yield is how much product was obtained, in this case 12.5 g of CCl₂F₂, and the theoretical yield is how much product could be obtained with the given reactants theoretically.

So we know already the actual yield, we need to <em>calculate the theoretical yield.</em>

First we need to <em>write the reaction chemical equation</em>:

CCl₄ + HF → CCl₂F₂ + HCl

and <em>balance the equation</em>:

CCl₄ + 2 HF → CCl₂F₂ + 2 HCl

In the equation we can see that <em>for every mol of CCl₄ we should get 1 mol of CCl₂F₂</em> (molar ratio 1:1). So if we <u>calculate the moles of CCl₄</u> in the given 39.2 g of CCl₄ we could know how many moles of CCl₂F₂ (assuming HF is in excess).

  • Moles of CCl₄ = mass CCl₄ / molar mass CCl₄
  • Molar Mass CCl₄ = 12.011 + 4 * 35.45 = 153.811 g/mol
  • Moles of CCl₄ = 39.2 g / 153.811 g/mol = 0.2549 moles

From the molar ratio we know:

Moles of CCl₂F₂ = moles of CCl₄ = 0.2549 moles

Now we need to <u>convert these moles into grams</u> to get the theoretical yield of CCl₂F₂ in grams:

  • mass CCl₂F₂ = moles CCl₂F₂ * molar mass CCl₂F₂
  • Molar Mass CCl₂F₂ = 12.011 + 2 * 35.45 + 2 * 18.998 = 120.907 g/mol
  • Mass CCl₂F₂ = 0.2549 moles * 120.907 g/mol = 30.81 g
  • Theoretical yield CCl₂F₂ = 30.81 g

Percent yield = (12.5 g / 30.81 g) * 100 = 40.6 %

8 0
3 years ago
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