SPM Chemistry

5.4 Hydrogen Bonds

1 Exercise

5.4 Hydrogen Bonding

5.5 Dative Bonds

1 Exercise

5.5 Dative Bonds

5.6 Metallic Bonds

1 Exercise

5.6 Metallic Bonds

5.7 Ionic and Covalent Compounds

1 Lesson | 1 Exercise

5.7.1 Properties of Ionic and Covalent Compounds

5.7 Properties of Ionic Compounds and Covalent Compounds

06 Acids, Bases and Salts

6.1 The Role of Water in Acidic and Basic Properties

3 Lessons | 1 Exercise

6.1.2 Bases and Alkali

6.1.3 The Role of Water in Acidic and Basic Properties

6.1 The role of water in showing acidity and alkalinity

6.2 Meaning of pH and Determination of pH

1 Lesson | 1 Exercise

6.2.1 Meaning of pH and Determination of pH

6.3 Strength of Acids and Alkalis

1 Lesson | 1 Exercise

6.3.1 Strength of Acids and Alkalis

6.3 Acid and Alkali Strength

6.4 Chemical Properties of Acids and Alkalis

3 Lessons | 1 Exercise

6.4.1 Chemical Properties of Acids

6.4.2 Chemical Properties of Alkalis

6.4.3 Writing Ionic Equation of The Reaction of Acids and Alkalies

6.4 Chemical Properties of Acids and Alkalis

6.5 Concentration of Aqueous Solution

2 Lessons | 1 Exercise

6.5.1 Concentration of Aqueous Solution

6.5.2 Molarity and Number of Moles

6.5 Concentration of Aqueous Solutions

6.6 Standard Solution

2 Lessons | 1 Exercise

6.6.1 Standard Solution

6.6 Standard Solutions

6.7 Neutralisation

2 Lessons | 1 Exercise

6.7.1 Neutralisation

6.7.2 Acid-Base Titration

6.7 Neutralization

6.8 Salts, Crystals and Their Uses in Daily Life

1 Lesson | 1 Exercise

6.8.1 Introduction to Salts

6.8 Salt, Crystals and Uses in Daily Life

6.9 Preparation of Salts

4 Lessons | 1 Exercise

6.9.1 Solubility of Salts, Oxide and Hydroxide

6.9.2 Preparing Salts

6.9.3 Preparing Soluble Salts

6.9.4 Preparing Insoluble Salts

6.9 Preparation of Salts

6.10 Action of Heat on Salts

2 Lessons | 1 Exercise

6.10.1 Identifying Gases

6.10.2 Effect of Heat on Salts

6.10 Action of Heat on Salt

6.11 Qualitative Analysis

3 Lessons | 1 Exercise

6.11.1 Colour of Salts

6.11.2 Identifying Anions

6.11.3 Identifying Cations

6.11 Qualitative Analysis

07 Rate of Reaction

7.1 Determining The Rate of Reaction

2 Lessons | 1 Exercise

7.1.1 Determining the Rate of Reaction

7.1.2 Analysing Rate of Reaction from Graph

7.1 Determining the Rate of Reaction

7.2 Factors Affecting the Rate of Reaction

1 Lesson | 1 Exercise

7.2.1 Factors Affecting the Rate of Reaction

7.2 Factors Affecting Reaction Rates

7.3 Applications of Factors that Affect the Rate of Reaction

1 Lesson | 1 Exercise

7.3.1 Applications of Factors that Affect the Rate of Reaction

7.3 Applications of Factors Affecting Reaction Rates in Life

7.4 The Collision Theory

1 Lesson | 1 Exercise

7.4.1 The Collision Theory

7.4 Collision Theory

08 Manufactured Substances in Industry

8.1 Alloys and Their Importance

1 Lesson | 1 Exercise

8.1.1 Alloys and Their Importance

8.1 Alloys and Their Importance

2 of 4

Previous Lesson

7.1 Determining the Rate of Reaction

Banner Advertisement

SPM Chemistry 7.1 Determining The Rate of Reaction 7.1 Determining the Rate of Reaction

Time limit: 0

Exercise Summary

0 of 10 Questions completed

Questions:

Information

You have already completed the exercise before. Hence you can not start it again.

Exercise is loading…

You must sign in or sign up to start the exercise.

You must first complete the following:

Results

Exercise complete. Results are being recorded.

Results

0 of 10 Questions answered correctly

Time has elapsed

You have reached 0 of 0 point(s), (0)

Earned Point(s): 0 of 0, (0)
0 Essay(s) Pending (Possible Point(s): 0)

Average score
Your score

Categories

Not categorized 0%

Would you like to submit your exercise result to the leaderboard?

Loading

Name: E-Mail:

Captcha:

captcha

maximum of 10 points
Pos.	Name	Entered on	Points	Result
Table is loading
No data available

1
2
3
4
5
6
7
8
9
10

Current
Review
Answered
Correct
Incorrect

Question 1 of 10

1. Question
1 point(s)
Which of the following correctly explains the meaning of average reaction rate?
- The average value of the rate of reaction that occurs over a certain period of time.
- The actual rate of reaction that occurs at a specific point or moment only.
- The slope of the tangent at any point along the curve of the graph.
- The rate of a reaction measured only at the moment the reaction begins to occur.
Correct

Incorrect
Question 2 of 10

2. Question
1 point(s)
How is the rate of a reaction at a given time (instantaneous rate) determined from a graph of quantity versus time?
- Takes the value of the quantity on the y-axis and divides it by the time on the x-axis.
- Calculates the area under the graph for the desired time period.
- Divides the total quantity of product by the total time.
- Find the slope of the tangent to the curve of the graph at that time.
Correct

Incorrect
Question 3 of 10

3. Question
1 point(s)
When is the rate of a reaction usually at its highest?
- When the graph begins to show a gradually increasing slope.
- Just before the reaction is complete and reaches equilibrium.
- At the beginning of the reaction (t = 0).
- When half of the reactants have been converted to products.
Correct

Incorrect
Question 4 of 10

4. Question
1 point(s)
Why does the rate of a reaction decrease as time goes by?
- The quantity of products formed prevents further reactions.
- The quantity or concentration of reactants decreases.
- The particle size of the reactants becomes larger during the reaction.
- The temperature of the system naturally decreases without external interference.
Correct

Incorrect
Question 5 of 10

5. Question
1 point(s)
In a graph of the mass of magnesium against time, what does the curve of the graph look like?
- The curve that decreases because the mass of the reactants decreases.
- The curve that increases because the magnesium gains weight during the reaction.
- The straight line is horizontal because the mass of the metal does not change in the chemical reaction.
- The curve, which initially rises, then drops sharply.
Correct

Incorrect
Question 6 of 10

6. Question
1 point(s)
What does it mean when the slope of the graph of quantity versus time becomes zero?
- The quantity of the reaction product has started to decrease again.
- The reaction has just started to slowly.
- The reaction is finished or complete.
- The reaction rate is at its maximum.
Correct

Incorrect
Question 7 of 10

7. Question
1 point(s)
Which is the correct formula for calculating the average rate over the time interval between t₁ and t₂?
- (Quantity at t₂ – Quantity at t₁) / (t₂ – t₁)
- (Quantity at t₂ + Quantity at t₁) / (t₂ + t₁)
- Slope of the tangent at the midpoint between t₁ and t₂
- (Total quantity of product) / (t₂ – t₁)
Correct

Incorrect
Question 8 of 10

8. Question
1 point(s)
In a graph of the volume of CO₂ gas against time, which part shows the slowest (but not yet zero) reaction rate?
- The steepest part of the curve at the beginning of the graph.
- The part of the graph where the line is a straight vertical line.
- The part of the curve that is the least steep before it becomes horizontal.
- The point where the tangent line has the greatest slope.
Correct

Incorrect
Question 9 of 10

9. Question
1 point(s)
What is the unit for the rate of reaction if the quantity of gas is measured in cm³ and the time in seconds?
- cm³/s
- s/cm³
- cm³ s
- g/cm³
Correct

Incorrect
Question 10 of 10

10. Question
1 point(s)
What is the main difference between the overall average rate and the average rate over a period of time t (from t = 0)?
- There is no difference between the two because both start from t = 0.
- The overall rate is always higher than the average rate at time t.
- The overall rate is calculated until the reaction is complete, while the rate at time t is calculated up to time t only.
- Overall rates use the tangential gradient, while rates at time t use tabular data.
Correct

Incorrect