Using the Equilibrium Constant
The reversible chemical reaction A+B?C+D
has the following equilibrium constant: Kc=[C][D][A][B]=5.9
Part A
Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?
Express the molar concentration numerically using two significant figures.
[A]= M
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Part B
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00M and [B] = 2.00M ?
Express the molar concentration numerically using two significant figures.
[D]= M
| Using the Equilibrium Constant The reversible chemical reactionA+B?C+D has the following equilibrium constant:Kc=[C][D][A][B]=5.9 | Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express the molar concentration numerically using two significant figures.
SubmitHintsMy AnswersGive UpReview Part Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00M and [B] = 2.00M ? Express the molar concentration numerically using two significant figures.
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Related questions
| Using the Equilibrium Constant The reversible chemical reactionA+B?C+D has the following equilibrium constant:Kc=[C][D][A][B]=5.9 | Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express the molar concentration numerically using two significant figures.
SubmitHintsMy AnswersGive UpReview Part Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00M and [B] = 2.00M ? Express the molar concentration numerically using two significant figures.
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