Question

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.

Answer 1

The mass of NaCl that reacted with the F₂ gas at 290 K and 1.5 atm is 132.6 g

Ideal gas law Equation & Stoichiometry

From the question, we are to determine the mass of NaCl that reacted with F₂

First, we will determine the number of moles of F₂ that reacted

From the ideal gas law equation, we have that

$n = \frac{PV}{RT}$

Where n is the number of moles

P is the pressure

V is the volume

R is the gas constant (R = 0.08206 L.atm.mol⁻¹.K⁻¹)

and T is the temperature in Kelvin

From the given information,

V = 18.0 L

T = 290 K

P = 1.5 atm

Putting the parameters into the equation, we get

$n = \frac{1.5 \times 18.0}{0.08206\times 290}$

n = 1.1346 moles

Now, we will determine the number of moles of NaCl that reacted with this amount of F₂ gas

From the given balaced chemical equation,

F₂ + 2NaCl → Cl₂ + 2NaF

This means, 1 mole of F₂ gas reacts completely with 2 moles of NaCl

Since

1 mole of F₂ gas reacts completely with 2 moles of NaCl

Then,

1.1346 moles of F₂ gas will react completely with 2×1.1346 moles of NaCl

2×1.1346 = 2.2692 moles

This is the number moles of NaCl that reacted

Now, for the mass of NaCl that reacted

From the formula,

Mass = Number of moles × Molar mass

Molar mass of NaCl = 58.44 g/mol

Mass of NaCl that reacted = 2.2692 × 58.44

Mass of NaCl that reacted = 132.6 g

Hence, the mass of NaCl that reacted with the F₂ gas at 290 K and 1.5 atm is 132.6 g

Part 2

To determine the mass of sodium chloride that can react with the same volume of fluorine gas at STP, follow the steps as shown above. But, we will change temperature and pressure to the standard temperature and pressure values. The standard temperature and pressure values are 273.15 K and 1.0 atm respectively.

Afterwards, we will then calculate the mass of sodium chloride needed by using the calculated number of moles and the formula as shown above.

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