A 1.87 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 820 mmHg . What is the partial pressure of excess reactant after the reaction occurs as completely as possible

This is an incomplete question, here is the complete question.

Chlorine gas reacts with fluorine gas to form chlorine trifluoride.

A 1.87 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 820 mmHg . What is the partial pressure of excess reactant after the reaction occurs as completely as possible?

Answer : The partial pressure of excess reactant after the reaction is, 62.6 mmHg

Explanation :

First we have to calculate the moles of

Using ideal gas equation:

where,

= partial pressure of = 337 mmHg = 0.443 atm

R = gas constant = 0.0821 L.mmHg/mol.K

T = temperature = 298 K

V = volume = 1.87 L

and,

where,

= partial pressure of = 820 mmHg = 1.08 atm

R = gas constant = 0.0821 L.atm/mol.K

T = temperature = 298 K

V = volume = 1.87 L

Now we have to calculate the limiting and excess reagent,

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 3 mole of react with 1 mole of

So, 0.0825 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Renaming moles of = 0.0338 - 0.0275 = 0.00630 mol

Now we have to calculate the partial pressure of excess reactant after the reaction.

Thus, the partial pressure of excess reactant after the reaction is, 62.6 mmHg

there all right good

explanation: