Chemistry, 12.07.2019 22:00 Jony4359

Hat mass of ethane, c2h6, contains the same number of molecules as 3.00 g of trichlorofluoromethane, ccl3f?

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Answer from: abieber4328

1. Calculate the molar masses of each compound:

$C_2H_6 = 12\cdot 2 + 1\cdot 6 = 30\ g/mol$

$CCl_3F = 12\cdot 1 + 35.5\cdot 3 + 19\cdot 1 = 137.5\ g/mol$

2. Both masses are referred to one mole of the substances. We can do a ratio between them and the 3 g of CCl_3F :

$\frac{30\ g\ C_2H_6}{137.5\ g\ CCl_3F} = \frac{x}{3\ g\ CCl_3F}\ \to\ x = \bf 0.654\ g\ C_2H_6$

Answer from: sierralynnbaldp16d4b

The mass of ${\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}$ is 0.654 g

Mole is a measure of the amount of substance. It is defined as the mass of a substance that has the same number of fundamental units as there are atoms in 12 g of carbon-12. Such fundamental units can be atoms, molecules or formula units.

Step1: Initially we have to calculate the moles of trichlorofluoromethane $\left({{\text{CC}}{{\text{l}}_{\text{3}}}{\text{F}}}\right)$

The formula to calculate the moles of trichlorofluoromethane $\left({{\text{CC}}{{\text{l}}_{\text{3}}}{\text{F}}}\right)$ is as follows:

${\text{Moles of CC}}{{\text{l}}_{\text{3}}}{\text{F}}=\frac{{{\text{Given mass of CC}}{{\text{l}}_{\text{3}}}{\text{F}}}}{{{\text{Molar mass of CC}}{{\text{l}}_{\text{3}}}{\text{F}}}}$ …… (1)

The given mass of $\left({{\text{CC}}{{\text{l}}_{\text{3}}}{\text{F}}}\right)$ is 3 g.

The molar mass of $\left({{\text{CC}}{{\text{l}}_{\text{3}}}{\text{F}}}\right)$ is 137.34 g/mol.

Substitute these values in equation (1)

$\align{{\text{Moles of CC}}{{\text{l}}_{\text{3}}}{\text{F}}{\bf&{=}}\left({3\;{\text{g}}}\right)\left({\frac{{{\text{1}}\;{\text{mol}}}}{{{\text{137}}{\text{.34}}\;{\text{g}}}}}\right)\cr&=0.02184\;{\text{mol}}\cr}$

The number of moles of trichlorofluoromethane $\left({{\text{CC}}{{\text{l}}_{\text{3}}}{\text{F}}}\right)$ is equal to the number of moles of ethane $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ and that is 0.02184 moles.

Step2: Calculate the mass of ethane $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ from the moles of ethane $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ .

The formula to calculate the moles of ethane $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ is as follows:

${\text{Moles of C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}=\frac{{{\text{Given mass of C}}{& _{\text{2}}}{{\text{H}}_{\text{6}}}}}{{{\text{Molar mass of C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}}$ …… (2)

The moles of $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ is 0.02184 mol.

The molar mass of $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ is 30 g/mol.

Substitute these values in equation (2)

$0.02184\;{\text{mol}}{\bf{=}}\left({{\text{Given mass of C}}{ & _{\text{2}}}{{\text{H}}_{\text{6}}}}\right)\left({\frac{{{\text{1}}\;{\text{mol}}}}{{{\text{137}}{\text{.34}}\;{\text{g}}}}}\right)$

(3)

Rearrange the equation (3) to calculate the mass of $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$

$\align{{\text{Given mass of }}{{\text{C}}_2}{{\text{H}}_6}&=\frac{{0.02184\;{\text{mol}}}}{{{\text{137}}{\text{.34}}\;{\text{g/mol}}}}\cr&=0.654\;{\text{g}}\cr}$

Hence, the mass of $\left({{\text{C}}{&_{\text{2}}}{{\text{H}}_{\text{6}}}}\right)$ is 0.654 g.

Learn more:

1. Bond energy of H-H bond in the given reaction:

2. The main purpose of conducting experiments:

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Mole concept

Keywords: stoichiometry, C2H6, CCL3F, moles, mass, molar mass, 0.02184 mol., 30 g/mol, 3 g, 137.34 g/mol and 0.654 g.

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since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

Answer from: Quest

Answer is to avoid experimental error

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