Worksheet: Kc to Kp Conversions

In this worksheet, we will practice converting between equilibrium constants defined by partial pressures and those defined by concentration.

Q1:

For the reaction H O ( ) H O ( ) 2 2 l g , 𝐾 = 0 . 1 2 2 P at 5 0 ∘ C . If partial pressures are measured relative to a standard pressure of 1 atm, what is the value of 𝐾 c at this temperature?

  • A 2 . 9 3 Γ— 1 0 βˆ’ 4
  • B 4 . 5 4 Γ— 1 0 βˆ’ 5
  • C 2 . 9 7 Γ— 1 0 βˆ’ 2
  • D 4 . 6 0 Γ— 1 0 βˆ’ 3
  • E0.122

Q2:

For the reaction N a S O Β· 1 0 H O ( ) N a S O ( ) + 1 0 H O ( ) 2 4 2 2 4 2 s s g , 𝐾 = 4 . 0 8 Γ— 1 0 P βˆ’ 2 5 at 2 5 ∘ C . If partial pressures are measured relative to a standard pressure of 1 atm, what is the value of 𝐾 c at this temperature?

  • A 2 . 7 1 Γ— 1 0 βˆ’ 4 8
  • B 4 . 6 6 Γ— 1 0 βˆ’ 5 9
  • C 3 . 0 9 Γ— 1 0 βˆ’ 2 8
  • D 5 . 3 1 Γ— 1 0 βˆ’ 3 9
  • E 4 . 0 8 Γ— 1 0 βˆ’ 2 5

Q3:

For the reaction H ( ) + I ( ) 2 H I ( ) 2 2 g g g , 𝐾 = 5 0 . 2 c at 4 4 8 ∘ C . If partial pressures are measured relative to a standard pressure of 1 bar, what is the value of 𝐾 P at this temperature?

Q4:

For the reaction N ( ) + 3 H ( ) 2 N H ( ) 2 2 3 g g g , 𝐾 = 0 . 5 0 c at 4 0 0 ∘ C . If partial pressures are measured relative to a standard pressure of 1 bar, what is the value 𝐾 P at this temperature?

  • A0.50
  • B 1 . 6 Γ— 1 0 βˆ’ 8
  • C 4 . 6 Γ— 1 0 βˆ’ 4
  • D 1 . 6 Γ— 1 0 βˆ’ 4
  • E 9 . 0 Γ— 1 0 βˆ’ 3

Q5:

What is the equation for the conversion of 𝐾 c to 𝐾 P for the reaction

  • A 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • B 𝐾 = 𝐾 𝑅 𝑇 P c
  • C 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • D 𝐾 = 𝐾 𝑅 𝑇 P c
  • E 𝐾 = 𝐾 P c

Q6:

What is the equation for the conversion of to for the following reaction?

  • A
  • B
  • C
  • D
  • E

Q7:

What is the equation for the conversion of 𝐾 c to 𝐾 P for the reaction

  • A 𝐾 = 𝐾 𝑅 𝑇 P c
  • B 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • C 𝐾 = 𝐾 𝑅 𝑇 P c
  • D 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • E 𝐾 = 𝐾 P c

Q8:

𝐾 c is equal to 0.28 for the following reaction at 9 0 0 ∘ C : Under standard conditions, all species have a concentration of 1.00 M and partial pressure of 1.00 atm. Calculate 𝐾 P for this reaction at 9 0 0 ∘ C .

  • A 2 . 6 Γ— 1 0 3
  • B 5 . 1 Γ— 1 0 βˆ’ 5
  • C 1 . 5 Γ— 1 0 3
  • D 3 . 0 Γ— 1 0 βˆ’ 5
  • E0.28

Q9:

What is the equation for the conversion of 𝐾 c to 𝐾 P for the reaction

  • A 𝐾 = 𝐾 𝑅 𝑇 P c
  • B 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • C 𝐾 = 𝐾 P c
  • D 𝐾 = 𝐾 𝑅 𝑇 P c
  • E 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2

Q10:

What is the equation for the conversion of 𝐾 c to 𝐾 P for the reaction

  • A 𝐾 = 𝐾 P c
  • B 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • C 𝐾 = 𝐾 𝑅 𝑇 P c
  • D 𝐾 = 𝐾 𝑅 𝑇 P c
  • E 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2

Q11:

What is the equation for the conversion of 𝐾 c to 𝐾 P for the reaction

  • A 𝐾 = 𝐾 P c
  • B 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2
  • C 𝐾 = 𝐾 𝑅 𝑇 P c
  • D 𝐾 = 𝐾 𝑅 𝑇 P c
  • E 𝐾 = 𝐾 ( 𝑅 𝑇 ) P c 2

Q12:

At 2 2 7 ∘ C , the following reaction has 𝐾 = 0 . 0 9 5 2 c : Under standard conditions, the concentration of each species is 1.00 M and the partial pressure is 1.00 bar. Calculate the value of 𝐾 P at 2 2 7 ∘ C for this reaction.

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