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)

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.

In a potential energy diagram, the difference between the potential energy of the products and the potential energy of the reactants is equal to the

activation energy of the forward reaction

activation energy of the reverse reaction

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

more water is added to the flask

the temperature is decreased to 15 o C

the temperature is increased to 35 o C

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

The frequency of collisions between atoms increases.

The mass of the sample decreases

The number of moles of gas increases.

The volume of each atom decreases.

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.

Kinetics and Equilibrium Review

Authored by Sydelle Steward

Chemistry

10th Grade - University

NGSS covered

Used 2+ times

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MULTIPLE CHOICE QUESTION

decreasing the concentration of H₂(g)

decreasing the pressure

increasing the concentration of N₂(g)

increasing the temperature

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

At 20.^oC, 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?

increasing the initial temperature to 25^oC

decreasing the concentration of HCl(aq) to 0.1 M

using 1.2 g of powdered Mg

using 2.4 g of Mg ribbon

Tags

NGSS.HS-PS1-5

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Kinetics and Equilibrium Review

Which term is defined as a measure of the disorder of a system?

Systems in nature tend to undergo changes toward

A 1.0-gram piece of zinc reacts with 5 milliliters of HCl(aq). Which of these conditions of concentration and temperature would produce the greatest rate of reaction?

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

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

Given the equation representing a reaction at equilibrium:
N₂(g) + 3H₂(g) <--> 2NH₃(g) + ENERGY
Which change causes the equilibrium to shift to the right?

At 20.^oC, 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?

Adding a catalyst to a chemical reaction results in

Given the potential energy diagram of a chemical reaction: . . . (see image)
Which arrow represents the potential energy of the reactants?

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

Access all questions and much more by creating a free account

Popular Resources on Wayground

Discover more resources for Chemistry

Kinetics and Equilibrium Review

Which term is defined as a measure of the disorder of a system?

Systems in nature tend to undergo changes toward

A 1.0-gram piece of zinc reacts with 5 milliliters of HCl(aq). Which of these conditions of concentration and temperature would produce the greatest rate of reaction?

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

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

Given the equation representing a reaction at equilibrium:N2(g) + 3H2(g) <--> 2NH3(g) + ENERGYWhich change causes the equilibrium to shift to the right?

At 20.oC, 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?

Adding a catalyst to a chemical reaction results in

Given the potential energy diagram of a chemical reaction: . . . (see image)Which arrow represents the potential energy of the reactants?

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

Access all questions and much more by creating a free account

Popular Resources on Wayground

Discover more resources for Chemistry

Given the equation representing a reaction at equilibrium:
N₂(g) + 3H₂(g) <--> 2NH₃(g) + ENERGY
Which change causes the equilibrium to shift to the right?

At 20.^oC, 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?

Given the potential energy diagram of a chemical reaction: . . . (see image)
Which arrow represents the potential energy of the reactants?

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