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

1 pts 2req

1. Calculate K: From Equilibrium C

2 Calculate K: From Initial One F... 1 pts 2req

3. Reaction Quobient True/False

4. Reaction Quotient Calculate

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5. Equilibrium Concentrations Calc

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Due Jun 22 at 11:55 PM

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Not Visited Is the reaction at equilibrium?

1 pts 2req

Consider the following reaction where K, = 77.5 at 600 K.

CO(g) + Cl₂(g)

CoCl₂(g)

A reaction mixture was found to contain 4.16x102 moles of CO(g), 4.05×102 moles of Cl₂(g) and 0.106 moles of COCI₂(g), in a 1.00 liter container.

[Review Topics]

[References]

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

If not, what direction must it run in order to reach equilibrium?

The reaction quotient, Qe equals

The reaction

A. must run in the forward direction to reach equilibrium.

B. must run in the reverse direction to reach equilibrium,

C. is at equilibrium.

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6/22/202/nHW 5-Calculations in Equilibrium Problems and LeChateller's Princ.

1 Calculate K From Equilibrium C

1 pts 2req

Calculate K. From Initial + One F

3 Reaction Quebent: True/False

Progress

ois groups

Due Jun 22 at 11:55 PM

Finish Assignment

1 pts/2req

4. Reaction Quotient Calculate

Preparation

Question

Question

Question

5. Equilibrium Concentrations Calc 1 pts req

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1 pts 2req

1 pts req

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The Reaction Quotient

Hi Q Search

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.

For a general reaction: aA+ bB cC + dD

K-([C] [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 deriote non-equilibrium concentrations.

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

Q

Q=K

Review Topics

Q> K

[References)

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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6/22/2023