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Radda [10]
3 years ago
11

What is the molarity of a solution containing 3.6 mol of KCl in 750 mL?

Chemistry
1 answer:
Vesnalui [34]3 years ago
4 0

Answer:

\boxed {\boxed {\sf 4.8 \ M \ KCl}}

Explanation:

The molarity of a solution is found by dividing the moles of solute by the liters. of solvent.

molarity=\frac{moles}{liters}

We know the solution has 3.6 moles of potassium chlorine. We know there are 750 milliliters of solvent, but we need to convert this to liters.

  • 1 liter is equal to 1000 milliliters. Set up a proportion.
  • \frac {1 \ L }{1000 \ mL}
  • Multiply by 750 mL and the units of mL will cancel.
  • 750 \ mL * \frac {1 \ L }{1000 \ mL} = \frac {750 \ mL}{1000 \ mL}= 0.75 \ L

Now we know the moles and liters, so we can calculate molarity.

  • moles= 3.6 mol KCl
  • liters= 0.75 L

Substitute these values into the formula.

molarity= \frac{3.6 \ mol \ KCl}{0.75 \ L}

Divide.

molarity= 4.8 \ mol \ KCl/ L

  • 1 mole per liter is equal to 1 molar.
  • Our answer of 4.8 moles of potassium chloride per liter is equal to 4.8 M KCl

molarity= 4.8 \ M \ KCl

The molarity of the solution is <u>4.8 M KCl.</u>

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Goryan [66]

Answer:

Kc = 2.34 mol*L

Explanation:

The calculation of the Kc of a reaction is performed using the values of the concentrations of the participants in the equilibrium.

A + B ⇄ C + D

Kc = [C] * [D] / [A] * [B]

According to the reaction

Kc = [SO2]^2 * [O2]^2 / [SO3]^2

Knowing the 0.900 mol of SO3 is placed in a 2.00-L it means we have a 0.450 mol/L of SO3

0.450 --> 0 + 0 (Beginning of the reaction)

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Explanation:

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gavmur [86]

Answer:

279.26K

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Answer:

N - 1s²2s²2p³

Explanation:

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The 2nd period tells us the principal energy level (a quantum number) is n = 2. Therefore, it must have already filled up the 1s sublevel.

The groups 13-18 on period 2 tells us that the 2s sublevel is also filled.

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Answer:

density=6.74g/ml

:320g÷47.5ml

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thank you

<em><u>I </u></em><em><u>hope</u></em><em><u> </u></em><em><u>this </u></em><em><u>is </u></em><em><u>helpful</u></em>

8 0
3 years ago
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