QuestionIdentify hydrocarbon $\mathrm{Q}$ if burning $1.00 \mathrm{~g}$ produces $3.22 \mathrm{~g}$ of CO₂. Options: A) cyclohexene B) cyclopentane C) ethene D) pentane.

Studdy Solution

STEP 1

Assumptions1. Substance Q is a hydrocarbon. . When1.00 g of Q is completely burned,3.22 g of carbon dioxide (CO) is produced.
3. The combustion of Q is complete and all the carbon in Q is converted to CO.
4. The molar mass of carbon (C) is approximately12 g/mol and the molar mass of carbon dioxide (CO) is approximately44 g/mol.

STEP 2

First, we need to find out how many moles of carbon are in the.22 g of CO2 produced. We can do this by dividing the mass of CO2 by its molar mass.
$Moles\, of\, CO2 = \frac{Mass\, of\, CO2}{Molar\, mass\, of\, CO2}$

STEP 3

Now, plug in the given values for the mass of CO2 and the molar mass of CO2 to calculate the moles of CO2.
$Moles\, of\, CO2 = \frac{3.22\, g}{44\, g/mol}$

STEP 4

Calculate the moles of CO2.
$Moles\, of\, CO2 = \frac{3.22\, g}{44\, g/mol} =0.073\, mol$

STEP 5

Since each molecule of CO2 contains one atom of carbon, the moles of carbon in CO2 is the same as the moles of CO2. Therefore, the moles of carbon in Q is also0.073 mol.

STEP 6

Now, we can find the mass of carbon in Q by multiplying the moles of carbon by the molar mass of carbon.
$Mass\, of\, carbon\, in\, Q = Moles\, of\, carbon \\times Molar\, mass\, of\, carbon$

STEP 7

Plug in the values for the moles of carbon and the molar mass of carbon to calculate the mass of carbon in Q.
$Mass\, of\, carbon\, in\, Q =0.073\, mol \\times12\, g/mol$

STEP 8

Calculate the mass of carbon in Q.
$Mass\, of\, carbon\, in\, Q =0.073\, mol \\times12\, g/mol =0.876\, g$

STEP 9

Now, we can find the percentage of carbon in Q by dividing the mass of carbon in Q by the total mass of Q and then multiplying by100%.
$Percentage\, of\, carbon\, in\, Q = \frac{Mass\, of\, carbon\, in\, Q}{Total\, mass\, of\, Q} \\times100\%$

STEP 10

Plug in the values for the mass of carbon in Q and the total mass of Q to calculate the percentage of carbon in Q.
$Percentage\, of\, carbon\, in\, Q = \frac{0.876\, g}{.00\, g} \\times100\%$

STEP 11

Calculate the percentage of carbon in Q.
$Percentage\, of\, carbon\, in\, Q = \frac{0.876\, g}{.00\, g} \\times100\% =87.6\%$

STEP 12

Now, we can compare this percentage with the percentage of carbon in each of the given hydrocarbons (A cyclohexene, B cyclopentane, C ethene, D pentane). The hydrocarbon with the closest percentage of carbon to87.6% is the likely identity of Q.
The percentage of carbon in each hydrocarbon is calculated as follows $Percentage\, of\, carbon\, in\, hydrocarbon = \frac{Number\, of\, carbon\, atoms \\times Molar\, mass\, of\, carbon}{Molar\, mass\, of\, hydrocarbon} \\times100\%$

STEP 13

For A cyclohexene (C6H10), the percentage of carbon is $Percentage\, of\, carbon\, in\, cyclohexene = \frac{6 \\times12\, g/mol}{82\, g/mol} \\times100\% =87.8\%$

STEP 14

For B cyclopentane (CH10), the percentage of carbon is $Percentage\, of\, carbon\, in\, cyclopentane = \frac{ \\times12\, g/mol}{70\, g/mol} \\times100\% =85.7\%$

STEP 15

For C ethene (C2H4), the percentage of carbon is $Percentage\, of\, carbon\, in\, ethene = \frac{2 \\times12\, g/mol}{28\, g/mol} \\times100\% =85.7\%$

STEP 16

For D pentane (C5H12), the percentage of carbon is $Percentage\, of\, carbon\, in\, pentane = \frac{5 \\times12\, g/mol}{72\, g/mol} \\times100\% =83.3\%$

STEP 17

Comparing these percentages, we see that cyclohexene (A) has the closest percentage of carbon (87.%) to the percentage of carbon in Q (87.6%). Therefore, the likely identity of Q is cyclohexene.
The identity of Q is likely cyclohexene (A).

Was this helpful?

Get Studdy

Scan QR code with your device to get Studdy on iOS or Android

QR code

Studdy solves anything!

Download the app

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

Parents Influencer program Contact Policy Terms