Chemistry Help?

Question

I'm kind of confused to if you could explain how to solve this that would be great! Thank you in advance!

Part 1. A chemist reacted 15.0 liters of F₂ gas with NaCl in the laboratory to form Cl₂ and NaF. Use the ideal gas law equation to determine the mass of NaCl that reacted with F₂ at 280. K and 1.50 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

Part 1:

Before we can solve for the mass of NaCl, we need to know the moles of F₂. Since F₂ is a gas, we can use the ideal gas law to do so: PV = nRT

V = 15.0 L T = 280 K P = 1.50 atm R = 0.0821 L*atm/mol*K

Rearrage PV=nRT to solve for n (moles)

n = PV/RT = (1.50 atm * 15.0 L) / (0.0821 L*atm/mol*K * 280K) = 0.97877 mol F₂

From the balanced chemical equation provided, we know that the molar ratio of F₂ to NaCl is 1:2. This means that for every 1 mole of F₂ that reacts, 2 moles of NaCl are required. We can use this molar ratio to solve for moles of NaCl:

2 mol NaCl / 1 mole F₂ = x mol NaCl / 0.97877 mol F₂

x = (2 mol NaCl)*(0.97877 mol F₂) / (1 mole F₂) = 1.9575 mol NaCl

Now we can use the molar mass (or molar weight) of NaCl to convert moles to grams:

MW_NaCl = 58.44 g/mol

(1.9575 mol NaCl) * (58.44 g NaCl / 1 mol NaCl) = 114.4 g NaCl

Round for significant digits and your final answer for Part 1 is 114 g NaCl.

Part 2:

You can repeat the process for Part 1 but change your T and P values to standard temperature and pressure (STP).

T = 273.15 K P = 1 atm

n = PV/RT = (1 atm * 15.0 L) / (0.0821 L*atm/mol*K * 273.15 K) = 0.66888 mol F₂

x = (2 mol NaCl)*(0.66888 mol F₂) / (1 mole F₂) = 1.3378 mol NaCl

(1.3378 mol NaCl) * (58.44 g NaCl / 1 mol NaCl) = 78.18 g NaCl

Round for sigfigs and your final answer for Part 2 is 78.2 g NaCl.