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

4. Reaction Quotient Calculate

Preparation

Question

Question

5 Equilibrium Concentrations Calc.

Progress

05 groups

Due Jun 22 at 11:55 PM

Finish Assignment

1 pts 2req

1 pts 2req

O

pts 2req

Not Vited The reaction quotient, Q. equals [

Consider the following reaction where K,

NH,Cl(s) NH3(g) + HCl(9)

A reaction mixture was found to contain 0.0572 moles of NH, C1(s), 0.00304 moles of NH3(g), and 0.00226 moles of HCl(g), in a 1.00 liter

container.

Is the reaction at equilibrium?

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

[Review Topics)

(References)

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

5.10 x 10-6 at 548 K

The reaction

O must run in the forward direction to reach equilibrium.

Omust run in the reverse direction to reach equilibrium.

O is at equilibrium.

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Save and Eat/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

67'

Partly sunny

1 pts 2req

1 pts req

Not Visited

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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ENG 940 m

7:21 AM

6/22/2023