Problem: Chlorine gas reacts with fluorine gas to form chlorine trifluoride.Cl2(g) + 3F2(g) → 2ClF3(g)A 2.00 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 784 mmHg .a. What is the pressure of ClF3 in the reaction vessel after the reaction?b. What is the total pressure in the reaction vessel after the reaction?

🤓 Based on our data, we think this question is relevant for Professor Stewart's class at UMD.

FREE Expert Solution

Reaction:            Cl2(g) + 3F2(g) → 2ClF3(g) 


Calculate moles of each reactant:

  • limiting reactant  forms less amount of product  determines max. amount of product


Ideal gas equation:


PV=nRTPVRT=nRTRTn=PVRTnCl2=(337 mm Hg×1 atm 760 mm Hg)2.00 L0.08206 L·atmmol·K298 K

nCl2 = 0.0363 mol Cl2


nF2=(784 mm Hg×1 atm 760 mm Hg)(2.00 L)(0.08206 L·atmmol·K)(298 K)

nF2 = 0.0844 mol F2


Mole to mole comparison:

  • 1 mol of Cl2 forms 2 moles ClF3


moles ClF3=0.0363 mol Cl2×2 mol ClF31 mol Cl2= 0.0726 mol

View Complete Written Solution
Problem Details

Chlorine gas reacts with fluorine gas to form chlorine trifluoride.

Cl2(g) + 3F2(g) → 2ClF3(g)

A 2.00 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 784 mmHg .

a. What is the pressure of ClF3 in the reaction vessel after the reaction?
b. What is the total pressure in the reaction vessel after the reaction?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Stewart's class at UMD.