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The reaction below has an equilibrium constant Kp=2.2Ã10^6 at 298 K. Calculate Kp Calculate Kp for the reaction below. 4COF2(g)â2CO2(g)+2CF4(g)for the reaction below.

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The reaction below has an equilibrium constant Kp=2.2Ã10^6 at 298K. 2COF2(g)âCO2(g)+CF4(g).Calculate Kp for the reaction below. COF2(g)â1/2CO2(g)+1/2CF4(g) Express your answer using two significant figures.

The reaction below has an equilibrium constant Kp=2.2x10^6 at 298K.
2COF2(g)<->CO2(g)+CF4(g)

Calculate Kp for the reaction below
2CO2(g)+2CF4(g)<->4COF2(g)

Express answer using two significant figures.

The reaction below has an equilibrium constant K_p=2.2Ã10⁶ at 298 K.
2COF₂(g)âCO₂(g)+CF₄(g)

Part A
Calculate K_p for the reaction below.
COF₂(g)â¹/₂CO₂(g)+¹/₂CF₄(g)

Part B
Calculate K_p for the reaction below.
²/₃COF₂(g)â¹/₃CO₂(g)+¹/₃CF₄(g)

Part C
Calculate K_p for the reaction below.
CO₂(g)+CF₄(g)â2COF₂(g)

Part D

Predict whether reactants or products will be favored at equilibrium for each of the above reactions.
Drag the appropriate items to their respective bins:
Reactants favored equilibrium OR Products favored equilibrium

²/₃COF₂(g) â ¹/₃CO₂(g)+¹/₃CF₄(g)
CO₂(g)+CF₄(g) â 2COF₂(g)
COF₂(g) â ¹/₂CO₂(g)+¹/₂CF₄(g)

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The reaction below has an equilibrium constant Kp=2.2Ã10^6 at 298 K. Calculate Kp Calculate Kp for the reaction below. 4COF2(g)â2CO2(g)+2CF4(g)for the reaction below.

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The reaction below has an equilibrium constant Kp=2.2Ã10^6 at 298 K. Calculate Kp Calculate Kp for the reaction below. 4COF2(g)â2CO2(g)+2CF4(g)for the reaction below.

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

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The reaction below has an equilibrium constant Kp=2.2Ã10^6 at 298 K. Calculate Kp Calculate Kp for the reaction below. 4COF2(g)â2CO2(g)+2CF4(g)for the reaction below.