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2 years ago

Isobutyl alcohol has a boiling point of 108.

1 answer:

3 0

You can determine the molar of an unknown solute from the boiling point elevation. When you do an experiment, add a certain known amount of the unknown compound to a solvent, say water. Then, determine the boiling point of the solution. The working equations would be the following:

Temp difference = Boiling pt of solution - Boiling point of pure solvent
Moles solute = (Temp difference)(Mass of solvent)/(Ebullioscopic constant of water)
Molar Mass = Mass of solute/Moles solute

The boiling point of water is 100°C,while the ebullioscopic constant is 0.512 °C/molal.

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A solution of cough syrup contains 5.00% active ingredient by volume. If the total volume of the bottle is 11.0 mL , how many mi

Marta_Voda [28]

All you need to do is change 5% into a decimal which would be 5/100 = .05
then multiply the decimal by the total volume to get the amount of active ingredients in ml
.05 * 56ml = 2.8 ml of active ingredient.

Hope that helps!

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2 years ago

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With the help of balanced chemical equation explain what happens when:(1)Zinc is put in dilute hydrochloric acid (2)Zinc is put

UkoKoshka [18]

Find the attached document.

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2 years ago

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If 4.59 g of potassium reacts with 3.6 g of sulfur according to the following reaction, how many grams of potassium sulfide can

EleoNora [17]

First convert the amount of grams you have of each substance to moles. Find your limiting reactant by calculating how many grams are needed to complete this reaction. If done correctly, you would see that we need .226 moles of Potassium to complete this reaction. However, we only have .118 moles of Potassium, so K must be our limiting reactant. Then use the moles of K to find out how many moles of K^2S are made. Then convert the amount of moles of K^2S to grams and you should get 10.3 g K^2S

8 0

2 years ago

A 0.200 M K 2SO 4 solution is produced by ________. dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L dissolving 43.6 g of K2SO4 in

Artist 52 [7]

A 0.200 M of K2SO4 solution is produced by diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL.

<u>Explanation</u>:

When dealing with dilution we will use the following equation:

M1 V1 = M2 V2

where,

M1 = initial concentration

V1 = initial volume

M2 = final concentration

V2 = final volume

By diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL, we get

M1 V1 = M2 V2

20.0 mL $\times$ 5.00 M = M2 $\times$ 500.0 mL

M2 = (20.0 mL $\times$ 5.00 M) / 500.0 mL

M2 = 0.200 M.

Hence A 0.200 M of K2SO4 solution is produced by diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL.

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2 years ago

Hikers have noticed that a sealed bag of potato chips puffs up when taken to the top of a mountain. Suppose that at the valley f

Dmitriy789 [7]

<h3>Answer:</h3>

0.95 atm

<h3>Explanation:</h3>

We are given;

Initial pressure, P1 = 1.0 atm

Initial temperature, T1 =298 K (25°C + 273)

Initial volume, V1 = 0.985 L

Final temperature, T2 = 295 K (22°C + 273)

Final volume, V2 = 1.030 L

We are required to find final air pressure;

Using the combined gas law;

$\frac{P1V1}{T1} =\frac{P2V2}{T2}$

To get, P2 ;

$P2=\frac{P1V1T2}{T1V2}$

$P2=\frac{(1.0)(0.985L)(295)}{(1.030)(298)}$

$P2 = 0.947 atm$

= 0.95 atm

Therefore, the air pressure at the top of the mountain is 0.95 atm

3 0

2 years ago

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