Fundamentals of Equilibrium

Pataasin ang iyong marka sa homework at exams ngayon gamit ang Quizwiz!

Which of the following best describes the term homogeneous equilibrium?

Homogeneous equilibrium is the equilibrium in a system in which all reactants and products are present in a single phase.

Consider the reaction below. If the initial concentration of the products C and D are both 0M, and at equilibrium the concentration of D increases by 0.037 M, how does the concentration of C change? 3A(g)+4B(g)⇋2C(g)+D(g)

It increases by 0.074 M

What will be the value of Kp in terms of Kc for the following equilibrium: A(g)+2B(g)→3C(g)+D(g)

Kc(RT)

Which of the following is NOT true regarding a system in equilibrium?

Only the concentration of the reactants is constant.

What will be the Kp for the following equilibrium: Cl2(l)→Cl2(g)

PCl2(g)

What is the reaction quotient for the reversible reaction shown below? P4(s)+5O2(g)⇌P4O10(s)

Qc = 1 / [O2]^5

The law of mass action best fits which of the following descriptions?

The law of mass action is the statement that the reaction quotient remains constant when a reversible reaction has attained equilibrium at a given temperature.

Find the reaction quotient for the reversible reaction below. 2CO2(g)⇌2CO(g)+O2(g)

[CO]^2[O2] / [CO2]^2

Write the expression for the reaction quotient in terms of concentration for the following reaction. 3H2+N2↽−−⇀2NH3

[NH3]^2 / [N2][H2]^3

Given the reaction below, what is the reaction quotient? 2KClO3(s)⇌2KCl(s)+3O2(g)

[O2]^3

An ICE chart is needed to calculate Kc if:

a combination of initial concentrations and at least one equilibrium concentration are given

Based on the reaction below, how will the concentration of D change if the concentration of C decreases by 0.053 M? 2A(aq)+5B(aq)⇋5C(aq)+D(aq)

decreases by .011 M

Q is always

dependent on the reaction and its progress.

Which type of equilibrium is more likely to omit substances from the equilibrium constant expression?

heterogeneous equilibria

As a reaction proceeds in the forward direction, Q will:

increase

Given the reaction below, how will the concentration of D change if the concentration of B decreases by 0.045 M? 3A(g)+2B(g)⇋2C(g)+5D(g)

increases by .113M

The value of the equilibrium constant, Kc, for a reaction will be __________.

independent of initial concentrations

When converting between Kc and Kp, this relationship will depend on the change in:

moles of gas between reactants and products

Substances on opposite sides of the equilibrium will have relative changes in concentration that are of:

opposite sign

Homogeneous equilibria will typically not exist in the:

solid phase

The relative changes in concentration of the substances involved in an equilibrium as the system equilibrates can be determined by looking at the:

stoichiometry of the equilibrium

Complete the set of algebraic terms representing the changes in concentrations for the following reaction: 2NO+O2 ⇌ 2NO2

x, 12x, −x

What will be the value of Kp in terms of Kc for the following equilibrium: 2A(g)+B(g)⇋3C(g)

Kc

The ideal gas constant is symbolized as:

R

Kc expressions will exclude:

solids

It can be difficult to differentiate a system at equilibrium from a system containing a:

very slow chemical reaction

Which of the following demonstrate homogeneous equilibria? (select all that apply)

- A reaction occurring in a liquid-phase solution - A reaction involving exclusively gaseous species - A reaction between solutes in liquid solution

Which of the following are true statements regarding reversible reactions?

- A reversible reaction might proceed in only one direction, with negligible contribution from the reverse reaction, depending on conditions. - The forward and reverse reactions may occur simultaneously.

The ideal gas law displays the relationship in which of the following? Select all that apply.

- Amontons's law - Charles's law - Boyle's law - Avogadro's law

Which of the following are reactions demonstrating heterogeneous equilibria? (select all that apply)

- Ca(OH)2(s)⇄Ca2+(aq)+2OH−(aq) - H2O(l)⇄H2O(g)

Identify the options below that are false about chemical equilibria. (select all that apply)

- Concentrations of products and reactants oscillate between a set range of values. - At equilibrium, all species have stopped reacting altogether.

Which of the following are examples of heterogeneous equilibria? (select all that apply)

- a reaction involving both gases and liquids - a reaction involving a solid and a liquid

For the following equilibrium: A+2B⇋C+3D If the change in concentration for B is 0.44 M, what will be the change in concentration for C?

-.22

For the following equilibrium: 2A+B→C+2D If the change in concentration for C is 0.36 M, what will be the change in concentration for A?

-.72

Consider the reaction described by the equation below. 4A(g)+5B(g)⇌5C(g)+2D(g) If the initial concentrations of A and B are both equal to 0.100M and the equilibrium concentration of B is 0.0840 M, what is the equilibrium concentration of D?

.0064 M

At equilibrium for the reaction in aqueous medium below, the concentrations of A, B, C, and D are 0.011 M, 0.0067 M, 0.0124 M, and 0.0062 M, respectively. What is the equilibrium constant? A+2B⇌3C+D

.024

Consider the reaction below. If the concentration of C decreases by 0.088 M, what will be the change in concentration for A? 2A(g)+3B(g)⇋5C(g)+4D(g)

.035 M

Consider the reaction below. At equilibrium, the concentration of A is 0.0502 M and the concentration of B is 0.057 M. If the equilibrium constant is Kc=3.8038, what is the equilibrium concentration of C? 2A(aq)+B(aq)⇌3C(aq)

.082 M

Consider the reaction below. If the concentration of B decreases by 0.068 M, what will be the change in concentration for C? 3A(g)+4B(g)⇋5C(g)

.085

Given the reaction below, if the concentration of B increases by 0.060 M, what will the be the change in concentration of A? 4A(g)+2B(g)⇋3C(g)+D(g)

.120 M

Based on the reaction below, if the concentration of B increases by 0.0830 M, what will be the change in concentration for A? 4A(g)+2B(g)⇋C(g)+2D(g)

.166

Based on the reaction below, if the concentration of D decreases by 0.0430 M, what will be the change in concentration for A ? 4A(g)+2B(g)⇋5C(g)+D(g)

.172 M

For the equilibrium C2H2+2Br2⇌C2H2Br4 if the initial concentrations are [C2H2]=0.80 M,[Br2]=1.60 M,[C2H2Br4]=0.55 M, and the reaction proceeds in the forward direction until equilibration, where [C2H2]=0.60 M, what is the final concentration (in units of molarity) of C2H2Br4?

.75 M

For the following equilibrium: 2A+B↽−−⇀C+2D If equilibrium concentrations are [A]=1.5 M, [C]=1.1 M, and [D]=0.68 M, and Kc=0.27, what is the equilibrium concentration of B?

.84 M

or the following equation, what is the equation for the reaction quotient? PCl3(l)+Cl2(g)⇌PCl5(s)

1 / [CL2]

For the following equilibrium: C2H2+2Br2⇌C2H2Br4 If the initial concentrations are: [C2H2]=0.25 M,[Br2]=0.50 M,[C2H2Br4]=2.5 M, and the reaction proceeds in the reverse direction until equilibration, where [C2H2Br4]=2.15 M, what is the final concentration of Br2?

1.2 M

What are possible algebraic terms representing the relative changes in concentrations for the following reaction? 2SO2+O2↔2SO3

2x, x, −2x


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