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Igoryamba
3 years ago
10

A hydrate is a compound that has water molecules within its crystal structure. Magnesium sulfate heptahydrate, MgSO4·7H2O, is a

hydrated form of magnesium sulfate. The hydrated compound has 7 moles of H2O for each mole of MgSO4. When 5.06 grams of MgSO4·7H2O are heated to at least 300.oC in a crucible by using a laboratory burner, the water molecules are released. The sample was heated repeatedly, until the remaining MgSO4 had a constant mass of 2.47 grams. During this laboratory activity, appropriate safety equipment was used and safety procedures were followed.Explain why the sample in the crucible was heated repeatedly until the sample had a constant mass.
Chemistry
1 answer:
Alenkasestr [34]3 years ago
4 0

Answer:

We are heating the sample repeatedly to become a pure compound of only MgSO4 (withot H2O) and a constant mass.

Explanation:

Step 1: Data given

Mass of MgSO4·7H2O = 5.06 grams

The remaining MgSO4 had a constant mass of 2.47 grams.

Step 2: Explain why the sample in the crucible was heated repeatedly until the sample had a constant mass.

Before heating the compound has magnesium sulfate and water.

The total mass of this compound is 5.06 grams

By heating we try to eliminate the water.

After heating there remain mgSO4 with a mass of 2.47 grams

This means 5.06 - 2.47 = 2.59 grams is water. All of this is eliminated.

The heating process happens repeatedly to make sure the final compound is pure. So the 2.47 grams os only MgSO4. If the mass would not be constant. It means the compound is not pure, the not all the water is eliminated yet.

So we are heating the sample repeatedly to become a pure compound of only MgSO4 (withot H2O) and a constant mass.

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The reaction of ethane gas (C2H6) with chlorine gas produces C2H5Cl as its main product (along with HCl). In addition, the react
Kazeer [188]

Answer:

The percent yield of  chloro-ethane in the reaction is 82.98%.

Explanation:

C_2H_6+Cl_2\rightarrow C_2H_5Cl+HCl

Moles of ethane = \frac{300.0 g}{30 g/mol}=10 mol

Moles of chlorine gases =\frac{650.0 g}{71 .0 g/mol}=9.1549 mol

As we can see that 1 mol of ethane react with 1 mole of chlorine gas.the 10 moles will require 10 mole of chlorine gas, but only 9.1549 moles of chlorine gas is present.

This means that chlorine gas is in limiting amount and amount of formation of chloro-ethane will depend upon amount of chlorine gas.

According to reaction , 1 mol of chloro ethane gives 1 mol of chloro-ethane.

Then 9.1549 moles of chlorien gas will give:

\frac{1}{1}\times 9.1549 mol=9.1549 mol of chloro-ethane

Mass of 9.1549 moles of chloro-ethane:

9.1549 mol × 64.5 g/mol = 590.4910 g

Theoretical yield of  chloro-ethane: 590.4910 g

Given experimental yield of chloro-ethane: 490.0 g

\% Yield=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

\%Yield (C_2H_5Cl)=\frac{490.0 g}{590.4910 g}\times 100=82.98\%

The percent yield of  chloro-ethane in the reaction is 82.98%.

6 0
3 years ago
Summary about helium
Zinaida [17]

Answer: Helium is an type of air that can be used to inflate balloons, balls,  and other things that require air. The carbon dioxide we breath out is similar to this helium.

Hope this helps!

6 0
3 years ago
Why are hydrophobic molecules such as fats and oils unable to dissolve in watery solutions?
Maru [420]
Hydrophobic mplecules are unable to fissolve in watery solution becuse they dislike water.

Hydro= water
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Hydrophobic= fear of water, or disliking water
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If your reply is "oil float to the top", then you're right. Oil and water DOES NOT mix together. Hope that help!
6 0
3 years ago
Three Stoichiometry Questions
andrezito [222]

Answer:

Explanation:

7)

Given data:

Mass of aluminium = 2.5 g

Mass of oxygen = 2.5 g

Mass of aluminium oxide = 3.5 g

Percent yield = ?

Solution:

Chemical equation:

4Al + 3O₂   →   2Al₂O₃

Number of moles of Al:

Number of moles = mass/ molar mass

Number of moles = 2.5 g/ 27 g/mol

Number of moles = 0.09 mol

Number of moles of oxygen:

Number of moles = mass/ molar mass

Number of moles = 2.5 g/ 32 g/mol

Number of moles = 0.08 mol

Now we will compare the moles of aluminium oxide with aluminium and oxygen.

                          Al         ;       Al₂O₃

                           4         :        2

                        0.09      :       2/4×0.09 = 0.045

                          O₂       :        Al₂O₃

                          3         :          2

                         0.08    :        2/3 ×0.08 = 0.053

The number of moles of aluminium oxide produced by Al are less so it will limiting reactant.

Mass of aluminium oxide:

Mass = number of moles × molar mass

Mass = 0.045  × 101.96 g/mol

Mass = 4.6 g

Percent yield:

Percent yield = actual yield / theoretical yield ×100

Percent yield = 3.5 g / 4.6 ×100

Percent yield = 76.1%

8)

Given data:

Mass of copper produced = 3.47 g

Mass of aluminium = 1.87 g

Percent yield = ?

Solution:

Chemical equation:

2Al + 3CuSO₄   →   Al₂(SO₄)₃ + 3Cu

Number of moles of Al:

Number of moles = mass/ molar mass

Number of moles = 1.87 g/ 27 g/mol

Number of moles = 0.07 mol

Now we will compare the moles of copper with aluminium.

                          Al         ;       Cu

                           2         :        3

                        0.07      :       3/2×0.09 = 0.105

             

Mass of copper:

Mass = number of moles × molar mass

Mass = 0.105  × 63.55 g/mol

Mass = 6.67 g

Percent yield:

Percent yield = actual yield / theoretical yield ×100

Percent yield =  3.47 g / 6.67 × 100

Percent yield = 52%

                       

4 0
3 years ago
Y’all know what a compound for chemistry is? pls h lo
Viefleur [7K]
Its two elements put together
3 0
3 years ago
Read 2 more answers
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