Question

A 100. mL reactor vessel is charged with 250. mg of P 4 and 4.21 atm of C l 2 at 298 K. The reaction goes to completion. How many moles of chlorine gas are initially in the vessel

Answer 1

There are 0.0172 moles of chlorine gas initially in the vessel.

Suppose we take a look and consider the reaction between P4 and Cl2, the balanced chemical equation between them can be expressed as:

$\mathbf{P_4 + 6 Cl _2 \to 4 PCl_3}$

Given that:

• mass of P₄ = 250 mg = 0.25g
• pressure of Cl₂ = 4.21 atm
• volume of the reactor = 100 mL = 0.1 L
• temperature = 298 K

Using the Ideal gas equation, the number of moles of chlorine gas that were initially present in the vessel is:

PV = nRT

Making (n) the subject of the formula:

$\mathbf{n = \dfrac{PV}{RT}}$

$\mathbf{n = \dfrac{4.21 \ atm \times 0.1 \ L}{0.0821 \ atm.L/mol*K \times 298 \ K}}$

n = 0.0172 moles

Therefore, we can conclude that there are 0.0172 moles of chlorine gas initially in the vessel.

Learn more about the Ideal gas equation here:

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