Part 1. A chemist reacted 18.0 liters of F2 gas with NaCl in the laboratory to form Cl2 gas and NaF. Use the ideal gas law equation to determine the mass of NaCl that reacted with F2 at 290. K and 1.5 atm. F2 + 2NaCl -> Cl2 + 2NaF

Part 2. Explain how you would determine the mass of sodium chloride that can react with the same volume of fluorine gas at STP. (10 points)​

= 93.264 grams NaCl(s)  

Explanation:

For the reaction given F₂(g) + 2NaCl(s) => 2NaF(s) + Cl₂(g), NaCl and NaF are in solid form at 290K (17°C) & 1.5atm pressure. Solids at these conditions do not have a volatile nature and the molar volume (Vm) = 0 Liters. Therefore the Ideal Gas Law is not applicable to solid NaCl or NaF.

A method most frequently used is the mole-mole ratio method. That is, convert all related data into moles, solve by ratio & proportion and convert to needed dimensions at end of problem.

For this problem:

 F₂(g) + 2NaCl(s) => 2NaF(s) + Cl₂(g)

Given Volume of F₂(g) = 18 Liters

Convert to moles F₂(g) by dividing volume given by 22.4 l/mole.

moles F₂(g) = 18L/22.4L/mol = 0.804mole F₂(g) in the 18L given,

Note rxn ratios between substances in the given reaction. In this case the reaction ratio between F₂(g) & NaCl(s) is 1 mole F₂ to 2 moles NaCl.

Set-up ratio & proportion equation and solve for unknown. The results will be in moles. If grams are needed multiply formula wt. by calculated moles to obtain results in terms of volume values.

that is ,,,

Rxn =>  1 mole F₂(g) to 2 moles NaCl

Calculated moles F₂(g) => 0.804 mole F₂(g)

Given moles of NaCl(s) => unknown (X)

From given rxn =>   1 mole F₂(g)  :  2 moles NaCl

Converted data => 0.804 mole F₂ : Unknown (X)

Setup ratio equation ...

1 mole F₂(g) / 0.804 mole F₂(g)  =  2 moles NaCl(s) / X

X = moles of NaCl from Rxn  

=> 1 · X = 2 · 0.804 moles NaCl(s) =  1.608 moles NaCl(s)

= 1.608 mole NaCl x 58 grams/mole = 93.264 grams NaCl(s)