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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

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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:

[tex]\mathbf{P_4 + 6 Cl _2 \to 4 PCl_3}[/tex]

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:

[tex]\mathbf{n = \dfrac{PV}{RT}}[/tex]

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

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:

https://brainly.com/question/18518493?referrer=searchResults

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