Please help!! 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.

1. PV = nRT. and solving for n (moles F2) we have

n = PV/RT = (1.50 atm)(15.0 L)/(0.0821 Latm/Kmol)(280K)

n = 0.9788 moles F2

mass NaCl = 0.9788 mol F2 x 2 mol NaCl x 58.4 g/mol = answer

Explanation:To find mass NaCl at STP just substitute 1 atm for pressure and 273K for temperature in the above equation and follow the rest of the calculations above.  

Explanation:

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

Volume of F2, V = 18 L

Temperature, T = 290K

Pressure, P = 1.5 atm

The equation of the reaction is given as;

F2 + 2NaCl → Cl2 + 2NaF

From the reaction, 1 mol of F2 reacted with 2 mol of NaCl

Using ideal gas equation to form number of moles of F2;

PV = nRT

n = PV / RT

n = 1.5 * 18 / (0.08205 * 290)

n = 27 / 23.7945

n = 1.135 mol

1 mol of F2 = 2 mol of NaCl

1.135 mol of F2 = x mol

x = 1.135 * 2 = 2.27 mol

We are to calculate mass;

Mass = Number of moles * Molar mass

Mass = 2.27 mol * 58.44 g/mol = 132.66 g

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

You would follow the same steps as in part 1. However, since this part has to deal with STP (Standard temperature and pressure) , you use the following values;

Temperature = 273 K

Pressure = 1 atm