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Lesson: Equilibrium Constants and Pressures

Worksheet • 9 Questions

Q1:

What is the pressure of C O 2 in an equilibrium gas mixture containing 0.45 atm of H 2 , 1.95 atm of H O 2 , and 0.95 atm of C O at 9 9 0 C ?

Q2:

What is the pressure of B r C l in an equilibrium mixture of C l 2 , B r 2 , and B r C l if the pressure of C l 2 in this mixture is 0.115 atm and the pressure of B r 2 is 0.450 atm?

  • A 4 . 9 × 1 0 2 atm
  • B 5 . 2 × 1 0 3 atm
  • C 20 atm
  • D 2 . 4 × 1 0 3 atm
  • E 4 . 1 × 1 0 2 atm

Q3:

One of the important reactions in the formation of smog is represented by the equation: In a gas mixture, the initial partial pressures of O 3 and N O are both equal to 1 . 2 × 1 0 8 atm. The partial pressures of all gases are 1.0 atm under standard conditions. Calculate the partial pressure of O 3 in the gas mixture at equilibrium.

  • A 4 . 9 × 1 0 2 6 atm
  • B 7 . 1 × 1 0 2 6 atm
  • C 1 . 4 × 1 0 2 6 atm
  • D 3 . 1 × 1 0 2 6 atm
  • E 7 . 9 × 1 0 2 6 atm

Q4:

What is the partial pressure of S 2 in an equilibrium mixture that results from the decomposition of H S 2 with an initial pressure of 0.824 atm? Assume that all pressures in 𝐾 P are expressed relative to a standard pressure of 1.00 atm and that changes in the pressure of H S 2 are small enough to be neglected.

Q5:

At 2 5 C and 1 atm, the partial pressures in an equilibrium mixture of N O 2 4 and N O 2 are 𝑃 ( N O ) 2 4 = 0.70 atm and 𝑃 ( N O ) 2 = 0.30 atm.

Nitrogen dioxide ( N O ) 2 dimerizes to form dinitrogen tetroxide ( N O ) 2 4 . How will the pressures of N O 2 and N O 2 4 change if the total pressure increases to 9.0 atm?

  • ABoth will increase.
  • BThey will both stay the same.
  • CBoth will decrease.
  • DThe partial pressure of N O 2 will decrease, while that of N O 2 4 will increase.
  • EThe partial pressure of N O 2 will increase, while that of N O 2 4 will decrease.

Calculate to 1 significant figure the equilibrium partial pressure of N O 2 at 9.0 atm and 2 5 C .

Q6:

Consider the reaction between H 2 and O 2 at 1 0 0 0 K. Under standard conditions, each species has a partial pressure of 1 atm. If a flask contains 0.500 atm of H 2 and 0.500 atm of O 2 , calculate the partial pressure of hydrogen at equilibrium.

  • A 8 . 6 7 × 1 0 atm
  • B 6 . 4 6 × 1 0 atm
  • C 9 . 0 5 × 1 0 atm
  • D 1 . 6 0 × 1 0 atm
  • E 0.500 atm

Q7:

Liquid N O 2 3 is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to N O and N O 2 . At 2 5 C , a value of 𝐾 P = 1.91 has been established for this decomposition. If 0.236 moles of N O 2 3 are placed in a 1.52-L vessel at 2 5 C , what is the equilibrium partial pressure of N O ( ) 2 3 g ?

Q8:

Nitrogen oxides are air pollutants produced by the reaction of nitrogen and oxygen at high temperatures. At 2 0 0 0 C , the value of the equilibrium constant for the reaction, N ( ) + O ( ) 2 N O ( ) 2 2 g g g , is 4 . 1 × 1 0 4 . Calculate the equilibrium concentration of N O ( ) g in air at 2 0 0 0 C if [ N ] 2 = 0.036 M and [ O ] 2 = 0.0089 M when equilibrium is reached.

  • A 3 . 6 × 1 0 4 M
  • B 8 . 1 × 1 0 6 M
  • C 1 . 3 × 1 0 7 M
  • D 0.78 M
  • E 0.88 M

Q9:

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 3 . 6 4 × 1 0 3 atm
  • BNot enough information has been provided.
  • C 4 . 0 8 × 1 0 2 5 atm
  • D 4 . 0 8 × 1 0 2 6 atm
  • E 24.4 atm
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