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san4es73 [151]
3 years ago
13

3mL of cyclohexanol (density = 0.9624 g/mL, Molecular weight = 100.158 g/mol) reacts with excess sulfuric acid to produce cycloh

exene (density = 0.811 g/mL, Molecular weight = 82.143 g/mol). What is the theoretical yield in Moles of cyclohexene? (hint: reaction scheme same as problem 1, 1:1 mole ratio) (10 pts)

Chemistry
2 answers:
Alex17521 [72]3 years ago
8 0

Answer:

The theoretical yield of moles cyclohexene is 0.0288 moles

Explanation:

Step 1: Data given

Volume of cyclohexanol = 3 mL

Density cyclohexanol = 0.9624 g/mL

Molar mass of cyclohexanol = 100.158 g/mol

Sulfuric acid is in excess

Density of cyclohexene = 0.811 g/mL

Molar mass of cyclohexene = 82.143 g/mol

Step 2: The balanced equation

C6H12O + H2SO4 → C6H10 + H3O + HSO4

Step 3: Calculate mass cyclohexanol

Mass cyclohexanol = density cyclohexane * volume

Mass cyclohexanol = 0.9624 g/mL * 3mL

Mass cyclohexanol = 2.8872 grams

Step 4: Calculate moles cyclohexanol

Moles cyclohexanol = mass cyclohexanol / molar mass

Moles cyclohexanol = 2.8872 grams / 100.158 g/mol

Moles cyclohexanol = 0.0288 moles

Step 5: Calculate moles cyclohexene

For 1 mol cyclohexanol we need 1 mol H2SO4 to produce 1 mol cyclohexene

For 0.0288 moles cyclohexanol we'll have 0.0288 moles cyclohexene

The theoretical yield of moles cyclohexene is 0.0288 moles

TiliK225 [7]3 years ago
4 0

Answer:

n_{C_6H_{10}}=0.03molC_6H_{10}

Explanation:

Hello,

In this case the undergoing chemical reaction is shown on the attached picture whereas cyclohexanol is converted into cyclohexene and water by the dehydrating effect of the sulfuric acid. Thus, for the starting 3 mL of cyclohexanol, the following stoichiometric proportional factor is applied in order to find the theoretical yield of cyclohexene in moles:

n_{C_6H_{10}}=3mLC_6H_{12}O*\frac{0.9624gC_6H_{12}O}{1mLC_6H_{12}O}*\frac{1molC_6H_{12}O}{100.158gC_6H_{12}O}*\frac{1molC_6H_{10}}{1molC_6H_{12}O} \\n_{C_6H_{10}}=0.03molC_6H_{10}

Besides, the mass could be computed as well by using the molar mass of cyclohexene:

m_{C_6H_{10}}=0.03molC_6H_{10}*\frac{82.143gC_6H_{10}}{1molC_6H_{10}} \\\\m_{C_6H_{10}}=2.4gC_6H_{10}

Even thought, the volume could be also computed by using its density:

V_{C_6H_{10}}=2.4gC_6H_{10}*\frac{1mLC_6H_{10}}{0.811gC_6H_{10}} \\V_{C_6H_{10}}=3mLC_6H_{10}

Best regards.

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When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 14.4 g of carbon were burned in the presence of
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Answer:

Mass of carbon dioxide produced = 52.8 g

Explanation:

Given data:

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3 years ago
W
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Answer:

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Explanation:

Given data:

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The net force on object is equal to the its mass multiply by its acceleration.

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If you added 45,000 calories to water that was at 25 degrees C, and the ending temperature was 35 degrees C, how much water did
user100 [1]

<u>Answer:</u>

<em>4.5 L water we have in litres (L).</em>

<em><u></u></em>

<u>Explanation:</u>

Q=m\times c \times \Delta T

where

\Delta T = Final T - Initial T

Q is the heat energy in calories

c is the specific heat capacity (for water 1.0  cal/(g℃))  

m is the mass of water

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3 years ago
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