A researcher is using 6.53 x 1023 molecules of chlorine gas (Cl2) in an experiment.

Question

A researcher is using 6.53 x 10²³ molecules of chlorine gas (Cl₂) in an experiment. How many grams of chlorine is the researcher using? Remember to include units (abbreviated appropriately) and the substance in your answer. Round your answer to the nearest 0.01.

Thanks in advance.

Answer 1

To determine the mass of chlorine gas (Cl₂) that the researcher is using, we need to know the molar mass of chlorine and the number of molecules provided.

The molar mass of chlorine (Cl₂) is approximately 35.45 grams/mole.

Given:

Number of molecules = 6.53 x 10^23 molecules

To calculate the mass of chlorine gas, we can use the following steps:

1. Convert the number of molecules to moles by dividing by Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol.

Moles of chlorine gas = Number of molecules / Avogadro's number

= 6.53 x 10^23 molecules / 6.022 x 10^23 molecules/mol

≈ 1.084 moles

2. Finally, calculate the mass of chlorine gas by multiplying the number of moles by the molar mass of chlorine.

Mass of chlorine gas = Moles of chlorine gas × Molar mass of chlorine

= 1.084 moles × 35.45 grams/mole

≈ 38.44 grams

Therefore, the researcher is using approximately 38.44 grams of chlorine gas (Cl₂) in the experiment.

Answer 2

First, you need the molar mass of chlorine. Since chlorine gas is diatomic, Cl₂, this will be ~ 71.0 g/mol

Now, using dimensional analysis, and knowing that there are 6.02 x 10²³ molecules in 1 mole, we can calculate the mass.

(71.0 g Cl₂/ 1 mol Cl₂) (1 mol Cl₂/ 6.02 x 10²³ molecules Cl₂) (6.53 x 10²³ molecules of Cl₂) = the mass, in grams, of Cl₂