Chemistry Practice Problems Gas Stoichiometry Practice Problems Solution: Xenon and fluorine will react to form binary compo...

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Solution: Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400°C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25°C. The reaction vessel is heated to 400°C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25°C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?

Problem

Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400°C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25°C. The reaction vessel is heated to 400°C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of Fat 25°C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?

Solution
  • We have to find the moles of Xe and F reacted to determine the empirical formula of this binary compound  XexFy. Reaction can be observed as:

Xe + F2 → XexFy + excess F2

  • We will be using the ideal gas equation to find the moles of Xe as well as F2 reacted
  • Freacted can be determined using the partial pressure and of F2 at start minus the partial pressure of the excess. Both will be using the same conditions in V and T

moles F2 reacted = moles F2 initial - moles F2 excess 

  • Calculating for the moles of Xe, F2 initial and F2 excess via Ideal gas equation:
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