{{asɛmtiNe Ɔkyerɛwfo}} | Nhomakorabea | Nneɛma a ɛma wotumi yɛ ade

2

A reaction is most likely to occur when reactant particles collide with

Proper energy, only

Proper orientation, only

Both proper energy and proper orientation

Neither proper energy nor proper orientation

2

Under what conditions will the rate of a chemical reaction always decrease?

The concentration of the reactants increases, and the temperature increases.

The concentration of the reactants increases, and the temperature decreases.

The concentration of the reactants decreases, and the temperature increases.

The concentration of the reactants decreases, and the temperature decreases.

2

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.
Zn (s) + 2 HCl (aq) --> H₂ (g) + ZnCl₂(aq)
Which set of reaction conditions produces H₂ at the fastest rate?

A 1.0 g lump of Zn (s) in 50. mL of 0.5 M HCl (aq) at 20 ^oC

A 1.0 g lump of Zn (s) in 50. mL of 0.5 M HCl (aq) at 30 ^oC

A 1.0 g of powdered Zn (s) in 50. mL of 1.0 M HCl (aq) at 20 ^oC

A 1.0 g of powdered Zn (s) in 50. mL of 1.0 M HCl (aq) at 30 ^oC

2

Increasing the temperature increases the rate of a reaction by:

Lowering the activation energy

Increasing the activation energy

Lowering the frequency of effective collisions between reacting molecules

Increasing the frequency of effective collisions between reacting molecules

2

For the reaction between aluminum metal and copper chloride (CuCl₂) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Breaking the aluminum into multiple pieces increases the concentration of aluminum

Breaking the aluminum into multiple pieces increases the surface area of aluminum exposed

Breaking the aluminum into multiple pieces is an exothermic process and will increase the temperature

2

Which solution of CuCl₂ will lead to the fastest reaction with aluminum?

5 g CuCl₂ in 50 mL

5 g CuCl₂ in 100 mL

10 g CuCl₂ in 50 mL

10 g CuCl₂ in 100 mL

An investigation was conducted to study the effect of the concentration of a reactant on the total time needed to complete a chemical reaction. Four trials of the same reaction were performed. In each trial the initial

concentration of the reactant was different. The time needed for the chemical reaction to be completed was measured. The data for each of the four trials are shown in the table below.

Use this data to answer questions 7-9.

null

2

State the effect of the concentration of the reactant on the rate of the chemical reaction above.

2

Explain your answer to 7 in terms of collision theory.

2

In a different experiment involving the same reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

1

How does pressure affect reation rate? Explain this in terms of collision theory

2

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.
A + B + heat --> C + D

Increasing the concentration of D

Increasing the concentration of A

Decreasing the temperature of the reaction

Use the reaction at equilibrium below to answer questions 12 and 13.

null

2

Which statement regarding this reaction at equilibrium is always true?

The rates of the forward and reverse reactions are equal.

The reaction occurs in an open system.

The reaction occurs in an closed system.

The concentrations of the reactants and the products are equal.

2

At constant temperature and pressure, an increase in the concentration of A(g) will cause

An increase in the concentration of B (g)

A decrease in the concentration of B (g)

A decrease in the concentration of C (g)

A decrease in the concentration of D (g)

Unit 6 Exam

Unit 6 Exam

A reaction is most likely to occur when reactant particles collide with

Under what conditions will the rate of a chemical reaction always decrease?

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.
Zn (s) + 2 HCl (aq) --> H₂ (g) + ZnCl₂(aq)
Which set of reaction conditions produces H₂ at the fastest rate?

Increasing the temperature increases the rate of a reaction by:

For the reaction between aluminum metal and copper chloride (CuCl₂) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl₂ will lead to the fastest reaction with aluminum?

State the effect of the concentration of the reactant on the rate of the chemical reaction above.

Explain your answer to 7 in terms of collision theory.

In a different experiment involving the same reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

How does pressure affect reation rate? Explain this in terms of collision theory

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.
A + B + heat --> C + D

Which statement regarding this reaction at equilibrium is always true?

At constant temperature and pressure, an increase in the concentration of A(g) will cause

A reaction is most likely to occur when reactant particles collide with

Under what conditions will the rate of a chemical reaction always decrease?

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.
Zn (s) + 2 HCl (aq) --> H₂ (g) + ZnCl₂(aq)
Which set of reaction conditions produces H₂ at the fastest rate?

Increasing the temperature increases the rate of a reaction by:

For the reaction between aluminum metal and copper chloride (CuCl₂) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl₂ will lead to the fastest reaction with aluminum?

State the effect of the concentration of the reactant on the rate of the chemical reaction above.

Explain your answer to 7 in terms of collision theory.

In a different experiment involving the same reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

How does pressure affect reation rate? Explain this in terms of collision theory

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.
A + B + heat --> C + D

Which statement regarding this reaction at equilibrium is always true?

At constant temperature and pressure, an increase in the concentration of A(g) will cause

Unit 6 Exam

Unit 6 Exam

A reaction is most likely to occur when reactant particles collide with

Under what conditions will the rate of a chemical reaction always decrease?

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.Zn (s) + 2 HCl (aq) --> H2 (g) + ZnCl2 (aq)Which set of reaction conditions produces H2 at the fastest rate?

Increasing the temperature increases the rate of a reaction by:

For the reaction between aluminum metal and copper chloride (CuCl2) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl2 will lead to the fastest reaction with aluminum?

State the effect of the concentration of the reactant on the rate of the chemical reaction above.

Explain your answer to 7 in terms of collision theory.

In a different experiment involving the same reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

How does pressure affect reation rate? Explain this in terms of collision theory

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.A + B + heat --> C + D

Which statement regarding this reaction at equilibrium is always true?

At constant temperature and pressure, an increase in the concentration of A(g) will cause

A reaction is most likely to occur when reactant particles collide with

Under what conditions will the rate of a chemical reaction always decrease?

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.Zn (s) + 2 HCl (aq) --> H2 (g) + ZnCl2 (aq)Which set of reaction conditions produces H2 at the fastest rate?

Increasing the temperature increases the rate of a reaction by:

For the reaction between aluminum metal and copper chloride (CuCl2) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl2 will lead to the fastest reaction with aluminum?

State the effect of the concentration of the reactant on the rate of the chemical reaction above.

Explain your answer to 7 in terms of collision theory.

In a different experiment involving the same reaction, it was found that an increase in temperature increased the rate of the reaction. Explain this result in terms of collision theory.

How does pressure affect reation rate? Explain this in terms of collision theory

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.A + B + heat --> C + D

Which statement regarding this reaction at equilibrium is always true?

At constant temperature and pressure, an increase in the concentration of A(g) will cause

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.
Zn (s) + 2 HCl (aq) --> H₂ (g) + ZnCl₂(aq)
Which set of reaction conditions produces H₂ at the fastest rate?

For the reaction between aluminum metal and copper chloride (CuCl₂) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl₂ will lead to the fastest reaction with aluminum?

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.
A + B + heat --> C + D

A student conducts an experiment where she reacts a lump of Zinc (Zn) with hydrocholoric acid (HCl). The balanced equation below represents the reaction.
Zn (s) + 2 HCl (aq) --> H₂ (g) + ZnCl₂(aq)
Which set of reaction conditions produces H₂ at the fastest rate?

For the reaction between aluminum metal and copper chloride (CuCl₂) that we performed together, what is the reason that breaking a single 5 g piece of aluminum into 25 smaller pieces of aluminum (still with a total mass of 5 g) speeds up the reaction rate.

Which solution of CuCl₂ will lead to the fastest reaction with aluminum?

Given the information below, which of the following changes will increase the rate of the forward reaction? Assume all reactants and products involved are in the gaseous form.
A + B + heat --> C + D