Chapter 17

Which of the following statements correctly describe how the addition of a catalyst will affect a system at equilibrium? Select all that apply.

A catalyst does not change the value of K. Equilibrium is unaffected.

Which of the following options correctly describe the equilibrium constant K? Select all that apply.

K expresses a particular ratio of equilibrium concentrations of products and reactants. The value of K is characteristic of a particular equilibrium system. K = kfwdkrevkfwdkrev for a system at equilibrium.

Why are the values of Q and K unitless? Multiple choice question.

The units of concentration are activities, which are the ratio of concentration of a substance to its standard-state concentration.

The equilibrium constant K for a system at equilibrium expresses a particular ratio of equilibrium constantBlank 1Blank 1 constant , Incorrect Unavailable of products and reactants at a particular temperatureBlank 2Blank 2 temperature , Correct Unavailable. The value of K is also equal to the ratio of the rate equalBlank 3Blank 3 equal , Incorrect Unavailable for the forward and reverse reactions.

1- Concerations 2- Temperature 3- Constants

Which of the following options correctly describe how a system at equilibrium will respond to a change in temperature? Select all that apply. Multiple select question. A change in temperature will cause a change in Kc.

A change in temperature will cause a change in Kc. If the forward reaction is exothermic, an increase in temperature causes a shift to the left.

Based on Le Chatelier's principle, in what ways can we optimize production of ammonia from the Haber process? Select all that apply. The reaction is N2 (g) + 3H2 (g) ⇌ 2NH3 (g); ΔHorxn = -91.8 kJ. Multiple select question.

Add N2 and H2 Remove NH3 Decrease the volume

Which of the following will change the pressure in a reaction involving only gases at equilibrium? Select all that apply

Changing the volume of the container Adding an inert gas Adding or removing a reactant or product

Which of the following statements correctly describe how a system at equilibrium will respond to a change in concentration of any species that appears in the expressions for Q and K? Select all that apply. Multiple select question.

If a reacting substance is added, the equilibrium position will shift to use up the substance. If a reactant is removed from the system, the equilibrium will shift toward the reactants. The value of Kc is not affected by changes in concentration.

Which of the following statements correctly describe how an equilibrium system containing gases will respond to changes in volume and/or pressure if the temperature remains unchanged? Select all that apply.

If the volume is decreased, the reaction shifts in the direction that produces fewer moles of gas. If the total number of moles of gas in the products and reactants is the same, a change in volume will not affect the equilibrium position. If an inert gas is added, there will be no effect on the equilibrium position.

A 1-L flask contains 0.50 mol SO2Cl2, 0.30 mol SO2, and 0.16 mol Cl2, which react according to the equation SO2Cl2 (g) ⇌ SO2 (g) + Cl2 (g), Kc = 0.011 for the reaction temperature. Select all the options that correctly interpret the data provided.

Kc = 0.011 =(0.30-x)(0.16-x)(0.50+x)(0.30-x)(0.16-x)(0.50+x) [SO2Cl2]eqm will be greater than 0.50 M. The reaction will proceed toward the reactant.

1.9 moles of HI are added to an evacuated, sealed 10.-L reaction vessel and allowed to decompose according to the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g); Kc = 1.26 × 10-3 Which of the following options correctly reflect how to calculate H2 at equilibrium? Select all that apply.

Kc = 1.26 × 10−3 = (0.19 − 2x)2x2Kc = 1.26 × 10-3 = (0.19 - 2x)2x2 If the change in [H2]H2 = +x, then at equilibrium [I2]I2 = x. The initial [HI]HI = 0.19 M.

A 1-L flask containing 1.0 mol Br2, 1.0 mol Cl2, and 2.0 mol BrCl react according to the equation Br2 (g) + Cl2 (g) ⇌ 2BrCl (g); Kc = 7.0 at the reaction temperature. Select all the options that correctly interpret the data provided.

Kc = 7.0 =(2.0+2x)2(1.0-x)(1.0-x)(2.0+2x)2(1.0-x)(1.0-x) The change in [Br2] will be -x.

Which of the following statements about the reaction quotient Q are correct? Select all that apply.

Q expresses a particular ratio of products and reactants at any time during a reaction. Q = K only at equilibrium. The expression for Q is the same as the expression for K.

Which of the following statements correctly describe a chemical system at equilibrium? Select all that apply.

The forward and reverse reactions occur at equal rates. There is no longer a change in concentration of reactants and products over time.

The Haber process is used to produce ammonia in industry. How does this process utilize Le Chatelier's principle to maximize reaction yields? The reaction is N2 (g) + 3H2 (g) ⇌ 2NH3 (g); ΔHorxn = -91.8 kJ.

The reaction is carried out at high pressures. Product is removed by condensation, so that the equilibrium continually shifts to the right to generate more product.

Which of the following statements correctly reflect Le Chatelier's principle? Select all that apply.

When a system at equilibrium is disturbed, the system reacts to minimize the effect of the disturbance. When a system at equilibrium is disturbed, Q ≠ K.

The law of mass action states that _____. Select all the options that complete the sentence correctly.

a chemical system reaches a state where the concentrations of reactants and products is a constant ratio equilibrium can be reached from any direction, i.e., by beginning with a mixture of reactants or products, or both

The law of mass action states that _____. Select all the options that complete the sentence correctly. Multiple select question.

a chemical system reaches a state where the concentrations of reactants and products is a constant ratio equilibrium can be reached from any direction, i.e., by beginning with a mixture of reactants or products, or both