CHEM 1A03 Chapter Notes - Chapter Unit 6 Module 2: Reaction Quotient, Chemical Equation, Lipophilicity

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Chemistry unit 6: module 2 solubility and chemical equilibrium ii. Q is a ratio of activities, a at any given time. Q depends on the balanced chemical equation. Q is large numerator is large, and there are lots of products at that point. Q is small numerator is small, and there are lots of reactants at that point. Des(cid:272)ri(cid:271)e the effe(cid:272)ti(cid:448)e (cid:272)on(cid:272)entration of ele(cid:272)trolytes in (cid:862)real(cid:863) or non-ideal situations. A unitless parameter that is obtained from a ratio of the concentration of a solute relative to its standard state (typically 1m) then multiplied by its activity coefficient (represented by gamma) Same ratio of reactants and products as q , except. The value tells us the extent to which the reaction has occred. Large value of k numerator is large and we have a lot of product reaction proceeding significantly to the right.

Related Questions

Learning Goal:

To determine equilibrium concentrations from initial conditions.

The reversible reaction

XY(aq)âX(aq)+Y(aq)

has a reaction quotient Qc defined as

Qc=[X][Y][XY]

Because the reaction is reversible, both the forward and reverse reactions will occur simultaneously. The reaction will eventually reach equilibrium, at which point the concentrations do not change, and Qc is equal to a constant known as Kc.

Part C

Based on a Kc value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

The reversible chemical reaction

A+BâC+D

has the following equilibrium constant:

Kc=[C][D]/[A][B]=7.5

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 your answer to two significant figures and include the appropriate units.

Part B

What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?

Express your answer to two significant figures and include the appropriate units.

Learning Goal:

To determine equilibrium concentrations from initial conditions.

The reversible reaction

XY(aq)âX(aq)+Y(aq)

has a reaction quotient Qc defined as

Qc=[X][Y]/[XY]

Calculating equilibrium concentrations when the net reaction proceeds forward

Consider mixture B, which will cause the net reaction to proceed forward.

Concentration (M)initial:change:equilibrium:[XY]0.500âx0.500âxnetââ[X]0.100+x0.100+x+[Y]0.100+x0.100+x

The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced.

Part B

Based on a Kc value of 0.180 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

Calculating equilibrium concentrations when the net reaction proceeds in reverse

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+xânetâ[X]0.300âx0.300âx+[Y]0.300âx0.300âx

The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.

Part C

Based on a Kc value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

Please, provide complete explanation.

CHEM 1A03 Chapter Notes - Chapter Unit 6 Module 2: Reaction Quotient, Chemical Equation, Lipophilicity

CHEM 1A03 Full Course Notes

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