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Delicious77 [7]
2 years ago
8

Which compound has the lowest melting point?

Chemistry
1 answer:
Natali5045456 [20]2 years ago
5 0

Answer:

K2O

Explanation:

If you use a melting point periodic table there is a listing of all the elements and their melting point.

Potassium (K) has a melting point of 63.25 degrees Celsius and oxygen (O) has a melting point of -218 degrees Celsius. Therefore, if you add those two values up

(63.25x2)+-218 = -91.5 Degrees Celsius

All the other compounds do not reach negatives.

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8. which change in state is associated with the heat of vaporization,
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The answer is 2, liquid to vapor because vaporization is the process of liquids to vapors.
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A chemist prepares a solution of iron(II) bromide (FeBr2) by measuring out 46. g of iron(II) bromide into a 400. mL volumetric f
schepotkina [342]

Solution

Given mass of FeBr2 = 85.5 g

Molar mass of FeBr2 = 215.65

No. of Moles of FeBr2 = Given Mass / Molar mass = 85.5 / 215.65

No. of Moles = 0.3964

Given Volume is 450 mL i.e. 0.450 L

Now Concentration = 0.3964/0.450

Hence Concentration = 0.881 mol/L

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Which is the correct Lewis structure for acetylene (C2H2)?
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What element is a gas at room temp, has 6 valence electrons, and is non-reactive
sveta [45]

Answer:

Noble gases

Explanation:

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7 0
3 years ago
Question 6 The mineral barite, (BaSO.) has a ke of 1.1 x 10" at 25°C. Calculate the solubility of barium sulfate in water, in: 6
Sav [38]

Explanation:

(6.1).    The reaction equation will be as follows.

             BaSO_{4}(s) \rightleftharpoons Ba^{2+}(aq) + SO^{2-}_{4}(aq)

Assuming the value of K_{sp} as 1.1 \times 10^{-10} and let the solubility of each specie involved in this reaction is "s". The expression for K_{sp} will be as follows.

            K_{sp} = [Ba^{2+}][SO^{-}_{2}]    (Solids are nor considered)

                        = s \times s

                   s = \sqrt{K_{sp}}

                      = \sqrt{1.1 \times 10^{-10}}

                      = 1.05 \times 10^{-5}

Therefore, solubility of barium sulfate in water is 1.05 \times 10^{-5}.

(6.2).   As the molar mass of BaSO_{4} is 233.38 g/mol

Therefore, the solubility is g/L will be calculated as follows.

                233.38 g/mol \times 1.05 \times 10^{-5}

                  = 2.45 \times 10^{-3} g/L

Therefore, solubility of barium sulfate in grams per liter is 2.45 \times 10^{-3} g/L.

8 0
3 years ago
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