2H 2 (g) + O 2 (g) → 2H 2 O(l) would be expected to have a faster reaction rate than Pb 2+ (aq) + S 2- (aq) → PbS(aq).

false, aqueous solutions already have the substance dissolved in it and the ions separated so there will be more effective collisions.

false, there is no way to make a valid prediction

Dynamic equilibrium is when

the rate of products being formed equals the rate of reactants being formed.

the rate of products being formed is greater than the rate of reactants being formed.

the rate of products being formed is less than the rate of reactants being formed.

concentration of products is equal to the concentration of reactants

When any reaction reaches equilibrium the c oncentration of reactants

are equal to the concentration of the products

A solution of propanone is in a covered container that is 1/2 full. Which description is the best?

both evaporation and condensation occur

neither evaporation and condensation occur

CO 2 (g) ↔ CO 2 (aq) What will increasing the the temperature of this system do to the solution equilibrium (saturated solution).

shift the equilibrium to the left favoring CO 2 (g) making it less soluble.

shift the equilibrium to the right favoring CO 2 (aq) making the gas more soluble.

2CO 2 (g) ↔ 2CO(g) + O 2 (g) In which direction will the equilibrium shift if the [CO 2 ] is increased and why?

to the right favoring the products because adding more CO 2 will make more effective collisions between the CO 2 molecules and therefore produce more CO and O 2 .

to the left favoring the reactants because adding more CO 2 will make less effective collisions between the CO 2 molecules and therefore produce less CO and O 2 .

2NH 3 (g) + 91.8 ↔ N 2 (g) + 3H 2 (g) Would an increase in temperature shift the equilibrium to the left or right and why?

right because there will be more effective collisions between the NH 3 molecules, therefore more products will be made.

left because their will be more effective collisions between the NH 3 molecules, therefore more products will be made.

left because their will be less effective collisions between the NH 3 molecules, therefore more products will be made.

H 2 (g) + Br 2 (g) + heat ↔ 2HBr(g) Which stresses will shift the equilibrium to the right?

Increasing temperature, increasing the [H 2 ], increasing the [Br 2 ], decreasing the [HBr]

Increasing, temperature, increasing the [H 2 ], increasing the [Br 2 ], decreasing the [HBr], increasing pressure

decreasing temperature, decreasing the [H 2 ], decreasing the [Br 2 ], increasing the [HBr]

Increasing temperature, decreasing the [H 2 ], increasing the [Br 2 ], increasing the [HBr]

CO 2 (s) + heat ↔ CO 2 (g) What effect will increasing the temperature have on the entropy of the system and why?

It will increase entropy because it will cause more effective collisions between the CO 2 (s) molecules causing it to sublime more and become a gas.

It will decrease entropy because it will cause more effective collisions between the CO 2 (s) molecules causing it to sublime more and become a gas.

It will increase entropy because it will cause less effective collisions between the CO 2 (s) molecules causing it to sublime more and become a gas.

The PE of the products is higher than the PE of the reactants. Which statement is true?

It is endothemic and exothermic.

It is neither endothemic and exothermic.

A(g) + B(g) ↔ AB(g) + 55.4 KJ If the activation energy for the forward reaction is 10 kJ, what is the activation energy for the reverse reaction?

There isn't enough information provided to calculate that.

2C(s) + H 2 (g) → C 2 H 2 (g) According to Reference Table I, this reaction is ______ and energy is ______.

both endothermic and exothermic, absorbed

neither endothermic and exothermic, constant

The dotted line represents

the lowered activation energy due to the addition of a catalyst.

the lowered activation energy due to the addition of an inhibitor.

the higher activation energy due to the addition of a catalyst.

the higher activation energy due to the addition of an inhibitor.

Topic VII: Kinetics and Equilibrium review

Authored by Barbara G

Chemistry

11th Grade - University

NGSS covered

Used 49+ times

Topic VII: Kinetics and Equilibrium review

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MULTIPLE CHOICE QUESTION

15 mins • 1 pt

How is ΔH determined?

H (PE)of reactants - H (PE) of products

H (PE) of reactants + H of (PE) products

H (PE) of products - H (PE) of reactants

H (PE) of products + H (PE) of reactants

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which describes an exothermic reaction?

ΔH is negative and the products have more potential energy than the reactants.

ΔH is negative and the products have less potential energy than the reactants.

ΔH is positive and the products have more potential energy than the reactants.

ΔH is positive and the products have less potential energy than the reactants.

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

CO₂(g) → CO₂(l) is

endothermic with increased entropy.

exothermic with increased entropy.

endothermic with decreased entropy.

exothermic with decreased entropy.

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

How many kJ of heat are absorbed when 2 mol of C₂H₄are formed?

157.2

26.2

52.4

104.8

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Activation energy is required for

only exothermic chemical reactions

only endothermic chemical reactions

all chemical reactions

both endothermic and exothermic chemical reactions

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

An inhibitor changes the rate of reaction by increasing the

activation energy and a catalyst changes the rate of reaction by increasing the activation energy.

potential energy and a catalyst changes the rate of reaction by increasing the activation energy.

activation energy and a catalyst changes the rate of reaction by lowering the activation energy.

activation energy and a catalyst changes the rate of reaction by lowering the potential energy.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which reaction will most likely occur spontaneously?

exothermic with decreased entropy

endothermic with increased entropy

exothermic with increased entropy

exothermic with decreased entropy

Tags

NGSS.HS-PS1-4

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Topic VII: Kinetics and Equilibrium review

How is ΔH determined?

Which describes an exothermic reaction?

CO₂(g) → CO₂(l) is

How many kJ of heat are absorbed when 2 mol of C₂H₄are formed?

Activation energy is required for

An inhibitor changes the rate of reaction by increasing the

Which reaction will most likely occur spontaneously?

Which shows a decrease in entropy for each change?

2H₂(g) + O₂(g) → 2H₂O(l) would be expected to have a faster reaction rate than Pb²⁺(aq) + S^2-(aq) → PbS(aq).

In a gaseous system, temperature remaining constant, an increase in pressure will

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Popular Resources on Wayground

Discover more resources for Chemistry

Topic VII: Kinetics and Equilibrium review

How is ΔH determined?

Which describes an exothermic reaction?

CO2(g) → CO2(l) is

How many kJ of heat are absorbed when 2 mol of C2H4 are formed?

Activation energy is required for

An inhibitor changes the rate of reaction by increasing the

Which reaction will most likely occur spontaneously?

Which shows a decrease in entropy for each change?

2H2(g) + O2(g) → 2H2O(l) would be expected to have a faster reaction rate than Pb2+(aq) + S2-(aq) → PbS(aq).

In a gaseous system, temperature remaining constant, an increase in pressure will

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

CO₂(g) → CO₂(l) is

How many kJ of heat are absorbed when 2 mol of C₂H₄are formed?

2H₂(g) + O₂(g) → 2H₂O(l) would be expected to have a faster reaction rate than Pb²⁺(aq) + S^2-(aq) → PbS(aq).