Just solve questions 7-10, thanks.1HgO(s) + 2 I−(aq) + H2O(l) ⇄ HgI2(g) + 2 OH−(aq) ; ∆H < 0Consider the equilibrium above. Which of the following changes will increase the concentration of HgI2?(A) Increasing the concentration of OH− (B) decreasing the pressure(C) Increasing the mass of HgO present (D) Increasing the temperature (E) Adding a catalyst2In which of the following systems would the equilibrium NOT be shifted by a change in the volume of the system at constant temperature?(A) CO(g) + NO(g) ⇄ CO2(g) + 1/2 N2(g) (B) N2(g) + 3 H2(g) ⇄ 2 NH3(g)(C) N2(g) + 2 O2(g) ⇄ 2 NO2(g) (D) N2O4(g) ⇄ 2 NO2(g) (E) NO(g) + O3(g) ⇄ NO2(g) + O2(g)3.What substance is missing in the following reaction mechanism?Step 1 NO + ___ à OONO Step 2 NO + OONO à 2NO2 Overall 2NO + O2 à 2NO2 (A) O2 (B) NO2 (C) NO (D) OONO4Relatively slow rates of chemical reaction are associated with which of the following?(A) The presence of a catalyst (B) High temperature (C) High concentration of reactants(D) Weak bonds in reactant molecules (E) High activation energy5Consider the potential energy diagram. Which of the followingis true for the reverse reaction?A. catalysed ∆Hrev= +50kJ Earev =+150kJB. catalysed ∆Hrev= -50kJ Ea=+50kJC. uncatalysed ∆Hrev= +50kJ Ea=+150kJD. uncatalysed ∆H= -50kJ Ea=+150kJ6Considering enthalpy and entropy, which of the following describes the reaction:A(g) + B(s) + kJ ↔ C(aq) + D(aq)A. the reaction goes forward C. the reaction goes in reverse B. the reaction will not proceed D. there will be an explosion E. the reaction is at equilibrium7Given that the reaction H3AsO4 + 3I−+ 2 H3O+ à H3AsO3 + I3− + H2O has a ka expression as follows:Ka = [H3AsO3][I3-] [I-]3[H3O]2If the concentration of H3AsO4 if increased...A) the equilibrium will shift to toward the products.B) the equilibrium will shift toward the reactantsC) there will be no shift in equilibrium.8Which statement concerning factors affecting rate of reaction is false?A. Decreasing the concentration of the reactants decreases the chance of collision.B. Decreasing the volume of a reaction flask containing gaseous reactants increases the chance of collision.C. A reaction occurs with every collision between particles.D. Increasing the temperature increases the reaction rate.9Equilibrium is a state of dynamic molecular behaviour, meaning that:A) the reaction eventually comes to a stop.B) reactants continually turn into products at a progressively slower rate.C) products continually turn into reactants at a progressively faster rate.D) reactants turn into products and products turn into reactants at different rates.E) reactants turn into products and products turn into reactants at equal rates.10Consider the reaction: Fe +3 + SCN - FeSCN (Yellow) (Red)Adding Fe(NO3)3(aq) to the above reaction will cause:A) the color to turn a deeper red because the equilibrium shifted to make more reactants.B) The color to turn a deeper red because the equilibrium shifted to make more products.C) The color to become a lighter yellow because the equilibrium shifted to make more reactants.D) The color to become a lighter yellow because the equilibrium shifted to make more products.E) None of the above are correct.

As per the request, the solution of Question number 7 to 10 are as follows:

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Just solve questions 7-10, thanks.

HgO_(s) + 2 I⁻_(aq) + H₂O_(l) ⇄ HgI_2(g) + 2 OH⁻_(aq); ∆H < 0

Consider the equilibrium above. Which of the following changes will increase the concentration of HgI₂?

(A) Increasing the concentration of OH⁻(B) decreasing the pressure

In which of the following systems would the equilibrium NOT be shifted by a change in the volume of the system at constant temperature?

(A) CO_(g) + NO_(g) ⇄ CO_2(g) + 1/2 N_2(g) (B) N_2(g) + 3 H_2(g) ⇄ 2 NH_3(g)

What substance is missing in the following reaction mechanism?

Step 1 NO + ___ à OONO

Step 2 NO + OONO à 2NO₂

Overall 2NO + O₂ à 2NO₂

(A) O₂ (B) NO₂ (C) NO (D) OONO

Relatively slow rates of chemical reaction are associated with which of the following?

(A) The presence of a catalyst (B) High temperature (C) High concentration of reactants

(D) Weak bonds in reactant molecules (E) High activation energy

Consider the potential energy diagram. Which of the following

is true for the reverse reaction?

A. catalysed ∆H_rev= +50kJ Ea_rev =+150kJ

B. catalysed ∆H_rev= -50kJ Ea=+50kJ

C. uncatalysed ∆H_rev= +50kJ Ea=+150kJ

D. uncatalysed ∆H= -50kJ Ea=+150kJ

Considering enthalpy and entropy, which of the following describes the reaction:

A_(g) + B_(s) + kJ ↔ C_(aq) + D_(aq)

A. the reaction goes forward C. the reaction goes in reverse

B. the reaction will not proceed D. there will be an explosion E. the reaction is at equilibrium

Given that the reaction H₃AsO₄ + 3I⁻+ 2 H₃O⁺ à H₃AsO₃ + I₃⁻ + H₂O has a ka expression as follows:

Ka = [H₃AsO₃][I₃^-]

[I-]³[H₃O]²

If the concentration of H₃AsO₄ if increased...

A) the equilibrium will shift to toward the products.

B) the equilibrium will shift toward the reactants

C) there will be no shift in equilibrium.

Which statement concerning factors affecting rate of reaction is false?

A. Decreasing the concentration of the reactants decreases the chance of collision.

B. Decreasing the volume of a reaction flask containing gaseous reactants increases the chance of collision.

C. A reaction occurs with every collision between particles.

D. Increasing the temperature increases the reaction rate.

Equilibrium is a state of dynamic molecular behaviour, meaning that:

A) the reaction eventually comes to a stop.

B) reactants continually turn into products at a progressively slower rate.

C) products continually turn into reactants at a progressively faster rate.

D) reactants turn into products and products turn into reactants at different rates.

E) reactants turn into products and products turn into reactants at equal rates.

Consider the reaction: Fe ⁺³ + SCN ^- FeSCN

(Yellow) (Red)

Adding Fe(NO₃)_3(aq) to the above reaction will cause:

A) the color to turn a deeper red because the equilibrium shifted to make more reactants.

B) The color to turn a deeper red because the equilibrium shifted to make more products.

C) The color to become a lighter yellow because the equilibrium shifted to make more reactants.

D) The color to become a lighter yellow because the equilibrium shifted to make more products.

E) None of the above are correct.

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