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5-Calculations in Equilibrium Problems and LeChatelier's Princ.

culate K From Equilibrium C

1 pts 2req

cutate K: From Initial One F

action Quotient Trae/False

paration

westion

estion

Reaction Quotient Calculate

Equilibrium Concentrations Calc

Progress:

0/5 groups

Due Jun 22 at 11:55 PM

Finish Assignment

1 pts 2req

1 pts 2req

O

1 pts 2req

1 pts 2seq

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Review Topics)

References]

Use the References to access important values if needed for this question.

Consider the following reaction where K-1.29-102 at 600 K:

COCI₂ (g)

CO (g) + Cl₂ (g)

A reaction mixture was found to contain 0.106 moles of COCI₂ (g), 4.35*102 moles of CO (g), and 4.05 102 moles of Cl₂ (g), in a 1.00 liter

container.

Indicate True (T) or False (F) for each of the following:

1. In order to reach equilibrium COCI₂(g) must be consumed.

2. In order to reach equilibrium K must decrease.

3. In order to reach equilibrium CO must be produced.

4. Q is greater than K

5. The reaction is at equilibrium. No further reaction will occur.

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HW 5-Calculations in Equilibrium Problems and LeChatelier's Princ.

Calculate K. From Equilibrium C

1 pts 2req

2 Calculate K From Initial One F 1 pts 2req

3 Reaction Quotient True/False

Question

Question

Question

Reaction Quotent Calculate

5 Equilibrum Concentrations Cale

Progress

05 groups

Due Jun 22 at 11:55 PM

Finish Assignment

1 pts 7req

Nek Subintted

1 pa 2req

1 pts 2req

Review Topics)

References]

The Reaction Quotient

The reaction quotient, Q, tells if a reaction is at equilibrium. It has the identical form as the equilibrium constant, K, but the concentrations used

are not necessarily the equilibrium concentrations.

Q

Q=K

Q> K

For a general reaction: aA+ bB cC + dD

#

K-(ICF (D))/(A) [B])

Q-((conc C) (conc D))/((conc A) (conc B))

For these problems we will use square brackets to denote equilibrium concentrations, and the term 'conc' to denote non-equilibrium concentrations

Both Q and K are a ratio of product concentrations over reactant concentrations. When:

Reactant concentrations are too high relative to product.

The reaction must run in the forward direction to reach equilibrium.

The reaction is at equilibrium.

No further changes will occur to reactant or product concentrations.

Product concentrations are too high relative to reactant.

The reaction must run in the reverse direction to reach equilibrium.

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