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

Calculate K. From Equilibrium Ca

1 pts 2req

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

1 pts req

3. Reaction Quotient True/False

Preparation

Question

Question

Question

Reaction Quotient Calculate

5. Equilibrium Concentrations Calc 1 pts req

Progress:

0's groups

Due Jun 22 at 11:55 PM

Jan 22

O

1 pls 2eq

Finish Assignment

[Review Topics

References)

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

Consider the following reaction where K₂=2.01 at 500 K:

PCl₂(g) + Cl₂(g) PCI,(g)

If the three gases are mixed in a rigid container at 500 K so that the partial pressure of each gas is initially one atm, what will happen?

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

1. A reaction will occur in which PCI,(g) is produced

2. K, will decrease.

3. A reaction will occur in which PCl, is consumed

4. Q is greater than K

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

Submit Answer

Retry Entire Group S more group attempts remaining

Cengage Learning Cengage Technical Support

Pandan

Email Instructor

Save and Exit

7:21 AM/n■ produt-cnow owl.cengagenow.com/um/takeAssignment/taketovalentActivity doſlocator assignment take

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.

Email Instructor

Next>

Save and Exit