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Worksheet: Calculating Reaction Quotients from Pressures

Q1:

Sodium sulfate decahydrate, N a S O · 1 0 H O 2 4 2 , dehydrates according to the equation In the equilibrium constant 𝐾 P , partial pressures are defined relative to a standard pressure of 1 atm. Calculate the partial pressure of water vapor at equilibrium with a mixture of N a S O · 1 0 H O 2 4 2 and N a S O 4 at 2 5 ∘ C .

  • A 24.4 atm
  • B 4 . 0 8 Γ— 1 0 βˆ’ 2 5 atm
  • C 4 . 0 8 Γ— 1 0 βˆ’ 2 6 atm
  • D 3 . 6 4 Γ— 1 0 βˆ’ 3 atm
  • ENot enough information has been provided.

Q2:

A sample of ammonium chloride was heated in a closed container. Ammonium chloride thermally decomposes according to the equation: At equilibrium, the pressure of N H ( ) 3 g was found to be 1.75 atm. Using a standard gas pressure of 1.00 atm, calculate the value of the equilibrium constant 𝐾 P for the decomposition at this temperature.

Q3:

Nitric oxide ( N O ) and chlorine react reversibly to form nitrosyl chloride ( N O C l ) according to the following equation: In a gas mixture at equilibrium, the partial pressures of N O , C l 2 and N O C l are 0.050 atm, 0.30 atm and 1.2 atm, respectively. Using a standard gas pressure of 1.0 atm, calculate the equilibrium constant 𝐾 P for this reaction.

  • A80
  • B96
  • C 5 . 2 Γ— 1 0 βˆ’ 4
  • D 1 . 9 Γ— 1 0 3
  • E 1 . 0 Γ— 1 0 βˆ’ 2