How many fluorine atoms are present in 45.3 g of C2F4?

Verified step by step guidance

Calculate the molar mass of \( \text{C}_2\text{F}_4 \) by adding the atomic masses of its constituent atoms: 2 carbon atoms and 4 fluorine atoms.

Determine the number of moles of \( \text{C}_2\text{F}_4 \) in 45.3 g by using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Use Avogadro's number \( (6.022 \times 10^{23} \text{ molecules/mol}) \) to find the number of molecules of \( \text{C}_2\text{F}_4 \) in the calculated moles.

Recognize that each molecule of \( \text{C}_2\text{F}_4 \) contains 4 fluorine atoms.

Multiply the number of \( \text{C}_2\text{F}_4 \) molecules by 4 to find the total number of fluorine atoms.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For C2F4, the molar mass is calculated by summing the atomic masses of its constituent elements: carbon (C) and fluorine (F). This value is essential for converting between grams and moles, which is necessary to determine the number of atoms in a given mass of the compound.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of particles (atoms, molecules, etc.) in one mole of a substance. This constant allows chemists to relate the macroscopic scale of substances (grams) to the microscopic scale (individual atoms or molecules). In this problem, it will be used to find the total number of fluorine atoms once the moles of C2F4 are determined.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. In the context of C2F4, stoichiometry helps determine the ratio of fluorine atoms to the moles of C2F4. Since each molecule of C2F4 contains four fluorine atoms, understanding this relationship is crucial for calculating the total number of fluorine atoms present in the given mass.

Recommended video:

Guided course

01:16

Stoichiometry Concept

Related Practice

Textbook Question

Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). a. CF₂Cl₂ c. C₂F₃Cl₃ d. CF₃Cl

views

Textbook Question

Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). b. CFCl₃

views

Textbook Question

How many bromine atoms are present in 12.8 g of CH2Br2?

Textbook Question

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. a. 1.245 g Ni, 5.381 g I

Textbook Question

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. b. 2.677 g Ba, 3.115 g Br

Textbook Question

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. c. 2.128 g Be, 7.557 g S, 15.107 g O

views