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

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

Kinetic and Equilibrium

Authored by Charles Martinez

Chemistry

10th Grade - University

NGSS covered

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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-PS1-5

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-PS1-6

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Kinetic and Equilibrium

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

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Kinetic and Equilibrium

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?