Based on the nature of the reactants in each of the equations below, which reaction at 25°C will occur at the fastest rate?

NaOH(aq) + HCl(aq) --> NaCl(aq) + H 2 O(l)

CH 3 OH(l) + CH 3 COOH(l) --> CH 3 COOCH 3 (aq) + H 2 O(l)

CaCO 3 (s) --> CaO(s) + CO 2 (g)

According to Table I, which equation represents a change resulting in the greatest quantity of energy released?

N 2 (g) + 3H 2 (g) --> 2NH 3 (g)

2C(s) + 3H 2 (g) --> C 2 H 6 (g)

2C(s) + 2H 2 (g) --> C 2 H 4 (g)

Which information about a chemical reaction is provided by a potential energy diagram?

the energy released or absorbed during the reaction

the oxidation states of the reactants and products

the average kinetic energy of the reactants and products

the change in solubility of the reacting substances

Given the equation representing a reaction: N 2 O 4 (g) <--> 2NO 2 (g) Which statement describes this reaction at equilibrium?

The concentration of N 2 O 4 (g) and the concentration of NO 2 (g) must be constant.

The concentration of N 2 O 4 (g) must equal the concentration of NO 2 (g).

The rate of the forward reaction is greater than the rate of the reverse reaction.

The rate of the reverse reaction is greater than the rate of the forward reaction.

A chemical reaction between iron atoms and oxygen molecules can only occur if

there are effective collisions between the particles

the atmospheric pressure decreases

Given the equation representing a system at equilibrium: N 2 (g) + 3H 2 (g) <--> 2NH 3 (g) + ENERGY Which changes occur when the temperature of this system is decreased ?

The concentration of H 2 (g) decreases and the concentration of NH 3 (g) increases.

The concentration of H 2 (g) increases and the concentration of N 2 (g) increases.

The concentration of H 2 (g) decreases and the concentration of N 2 (g) increases.

The concentration of H 2 (g) decreases and the concentration of NH 3 (g) decreases.

Given the equation representing a closed system: N 2 O 4 (g) <--> 2NO 2 (g) Which statement describes this system at equilibrium?

The rate of the forward reaction and the rate of the reverse reaction are equal.

The volume of the NO 2 (g) is greater than the volume of the N 2 O 4 (g).

The volume of the NO 2 (g) is less than the volume of the N 2 O 4 (g).

The rate of the forward reaction and the rate of the reverse reaction are unequal.

Given the balanced equation representing a reaction: 2H 2 O(l) + 571.6 kJ → 2H 2 (g) + O 2 (g) What occurred as a result of this reaction?

Energy was absorbed, and entropy increased.

Energy was absorbed, and entropy decreased.

Energy was released, and entropy increased.

Energy was released, and entropy decreased.

Systems in nature tend to undergo changes toward

lower energy and higher entropy

higher energy and lower entropy

higher energy and higher entropy

Which expression represents the ΔH for a chemical reaction in terms of the potential energy, PE, of its products and reactants?

PE of products - PE of reactants

PE of products + PE of reactants

PE of products × PE of reactants

PE of products ÷ PE of reactants

Which factors must be equal in a reversible chemical reaction at equilibrium?

the rates of the forward and reverse reactions

the activation energies of the forward and reverse reactions

the concentrations of the reactants and products

the potential energies of the reactants and products

For a given reaction, adding a catalyst increases the rate of the reaction by

providing an alternate reaction pathway that has a lower activation energy

providing an alternate reaction pathway that has a higher activation energy

using the same reaction pathway and increasing the activation energy

using the same reaction pathway and decreasing the activation energy

Given the equation representing a reaction at equilibrium: N 2 (g) + 3H 2 (g) <--> 2NH 3 (g) + ENERGY Which change causes the equilibrium to shift to the right?

increasing the concentration of N 2 (g)

decreasing the concentration of H 2 (g)

At 20. o C, a 1.2-gram sample of Mg ribbon reacts rapidly with 10.0 milliliters of 1.0 M HCl(aq). Which change in conditions would have caused the reaction to proceed more slowly?

decreasing the concentration of HCl(aq) to 0.1 M

increasing the initial temperature to 25 o C

Adding a catalyst to a chemical reaction results in

a decrease in activation energy and an increase in the reaction rate

a decrease in activation energy and a decrease in the reaction rate

an increase in activation energy and a decrease in the reaction rate

an increase in activation energy and an increase in the reaction rate

Given the reaction at equilibrium: 2SO 2 (g) +O 2 (g) <--> 2SO 3 (g) + HEAT Which change will shift the equilibrium to the right?

decreasing the amount of SO 2 (g)

decreasing the amount of O 2 (g)

What occurs when the temperature is increased in a system at equilibrium at constant pressure?

The rate of the endothermic reaction increases.

The rate of the forward reaction increases, and the rate of the reverse reaction decreases.

The rate of the forward reaction decreases, and the rate of the reverse reaction increases.

The rate of the exothermic reaction decreases.

Which statement about a system at equilibrium is true?

The forward reaction rate is equal to the reverse reaction rate.

The forward reaction rate is less than the reverse reaction rate.

The forward reaction rate is greater than the reverse reaction rate.

The forward reaction rate stops and the reverse reaction rate continues.

The activation energy required for a chemical reaction can be decreased by

adding a catalyst to the reaction

increasing the surface area of the reactant

increasing the temperature of the reactant

A catalyst increases the rate of a chemical reaction by

lowering the activation energy of the reaction

. lowering the potential energy of the products

raising the temperature of the reactants

raising the concentration of the reactants

Given the reaction: N 2 (g) +O 2 (g) +182.6 KJ <--> 2 NO(g) Which change would cause an immediate increase in the rate of the forward reaction?

increasing the concentration of N 2 (g)

increasing the concentration of NO(g)

decreasing the reaction temperature

decreasing the reaction pressure

Which statement must be true about a chemical system at equilibrium?

The rate of the forward reaction is equal to the rate of the reverse reaction.

The forward and reverse reactions stop.

The concentration of reactants and products are equal.

The number of moles of reactants is equal to the number of moles of product.

Which statement best describes a chemical reaction when it reaches equilibrium?

The forward and reverse reaction rates are the same.

The concentrations of reactants and products are the same.

The concentrations of the reactants decrease to zero.

The forward reaction rate decreases to zero.

Kinetics and Equilibrium TICKET

Authored by Sydelle Steward

Chemistry

10th Grade - University

NGSS covered

Used 39+ times

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53 questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which list of the phases of H₂O is arranged in order of increasing entropy?

ice, steam, and liquid water

ice, liquid water, and steam

steam, liquid water, and ice

steam, ice, and liquid water

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

An open flask is half filled with water at 25^oC. Phase equilibrium can be reached after

more water is added to the flask

the flask is stoppered

the temperature is decreased to 15^oC

the temperature is increased to 35^oC

Tags

NGSS.HS-PS3-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Given the equation for a system at equilibrium:
N₂(g) + 3H₂(g) <--> 2NH₃(g) + energy
If only the concentration of N₂(g) is increased, the concentration of

NH₃(g) increases

NH₃(g) remains the same

H₂(g) increases

H₂(g) remains the same

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Given the reaction at equilibrium:
C₂ + D₂(g) <-->2 CD(g) + energy
Which change will cause the equilibrium to shift?

increase in pressure

increase in volume

addition of heat

addition of a catalyst

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Given the accompanying potential energy diagram for a reaction:
Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the sample is increased?

The mass of the sample decreases

The number of moles of gas increases.

The volume of each atom decreases.

The frequency of collisions between atoms increases.

Tags

NGSS.HS-PS3-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Given the equation representing a reaction at equilibrium:
2SO₂(g) + O₂(g) <--> 2SO₃(g) +HEAT
Which change causes the equilibrium to shift to the right?

adding a catalyst

adding more O₂(g)

decreasing the pressure

increasing the temperature

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

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Kinetics and Equilibrium TICKET

Which list of the phases of H₂O is arranged in order of increasing entropy?

An open flask is half filled with water at 25^oC. Phase equilibrium can be reached after

Given the equation for a system at equilibrium:
N₂(g) + 3H₂(g) <--> 2NH₃(g) + energy
If only the concentration of N₂(g) is increased, the concentration of

Given the reaction at equilibrium:
C₂ + D₂(g) <-->2 CD(g) + energy
Which change will cause the equilibrium to shift?

Given the accompanying potential energy diagram for a reaction:
Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?

A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the sample is increased?

Given the equation representing a reaction at equilibrium:
2SO₂(g) + O₂(g) <--> 2SO₃(g) +HEAT
Which change causes the equilibrium to shift to the right?

Given the potential energy diagram for a chemical reaction:
(see image)
Which numbered interval represents the heat of reaction?

The solid and liquid phases of water can exist in a state of equilibrium at 1 atmosphere of pressure and a temperature of

In most aqueous reactions as temperature increases, the effectiveness of collisions between reacting particles

Access all questions and much more by creating a free account

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Kinetics and Equilibrium TICKET

Which list of the phases of H2O is arranged in order of increasing entropy?

An open flask is half filled with water at 25oC. Phase equilibrium can be reached after

Given the equation for a system at equilibrium:N2(g) + 3H2(g) <--> 2NH3(g) + energyIf only the concentration of N2(g) is increased, the concentration of

Given the reaction at equilibrium: C2 + D2(g) <-->2 CD(g) + energyWhich change will cause the equilibrium to shift?

Given the accompanying potential energy diagram for a reaction:Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?

A sample of helium gas is in a sealed, rigid container. What occurs as the temperature of the sample is increased?

Given the equation representing a reaction at equilibrium:2SO2(g) + O2(g) <--> 2SO3(g) +HEATWhich change causes the equilibrium to shift to the right?

Given the potential energy diagram for a chemical reaction:(see image)Which numbered interval represents the heat of reaction?

The solid and liquid phases of water can exist in a state of equilibrium at 1 atmosphere of pressure and a temperature of

In most aqueous reactions as temperature increases, the effectiveness of collisions between reacting particles

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Which list of the phases of H₂O is arranged in order of increasing entropy?

An open flask is half filled with water at 25^oC. Phase equilibrium can be reached after

Given the equation for a system at equilibrium:
N₂(g) + 3H₂(g) <--> 2NH₃(g) + energy
If only the concentration of N₂(g) is increased, the concentration of

Given the reaction at equilibrium:
C₂ + D₂(g) <-->2 CD(g) + energy
Which change will cause the equilibrium to shift?

Given the accompanying potential energy diagram for a reaction:
Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants?

Given the equation representing a reaction at equilibrium:
2SO₂(g) + O₂(g) <--> 2SO₃(g) +HEAT
Which change causes the equilibrium to shift to the right?

Given the potential energy diagram for a chemical reaction:
(see image)
Which numbered interval represents the heat of reaction?