Question

Consider the following reaction in which all reactants and products are gases.


P4+6Cl2⟶4PCl3

A 100. ML reactor vessel is charged with 250. Mg of P4 and 4. 21 atm of Cl2 at 298 K. The reaction goes to completion.

How many moles of chlorine gas are initially in the vessel?

Answer 1

Based on the equation of the reaction, the moles of chlorine gas initially in the vessel is 0.12 moles

How many moles of chlorine were initially present?

The moles of chlorine initially present is determined using the equation of the reaction:

• P4 + 6 Cl2 ⟶ 4 PCl3

At STP, 1 mole of P4 reacts with 6 moles of chlorine.

Molar mass of P4 = 124.0 g

Molar mass of chlorine = 71.0 g

Mass of P4 in reaction vessel = 250 mg = 0.25g

moles of P4 in 0.25 g = 0.25/124 = 0.02 moles

0.02 moles of P4 will react with 0.02 × 6 moles of chlorine = 0.12 moles of chlorine.

Therefore, the moles of chlorine gas initially in the vessel is 0.12 moles.

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