IB Grade 12 Chemistry by Pavan | Practice Test to Test Your Knowledge
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  3. IB Grade 12 Chemistry
IB Grade 12 Chemistry

IB Grade 12 Chemistry

Thorough mock test covering scientific inquiry, experimental design, and conceptual understanding. Includes laboratory skills, data analysis, and interdisciplinary scientific applications.

2025-07-22
Pavan Pavan
IB Class 12 Chemistry Grade 12

Duration

30 min

Questions

30

Marking

Negative

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Questions Preview

What is the definition of a mole in chemistry?

A
The amount of substance containing 6.02 × 10²³ particles
B
The mass of a substance in grams
C
The amount of substance in liters
D
The volume of a gas at STP

What is Avogadro's constant?

A
6.02 × 10²³ particles per mole
B
1.00 × 10³ particles per mole
C
6.00 × 10²³ particles per gram
D
1.00 × 10²⁴ particles per mole

The molar mass of a substance is the mass of one mole of that substance. What is the molar mass of Carbon (C)?

A
12.01 g/mol
B
16.00 g/mol
C
14.00 g/mol
D
1.01 g/mol

Which of the following is true about the relationship between moles, mass, and molar mass?

A
Number of moles = Mass / Molar Mass
B
Molar Mass = Number of moles × Mass
C
Mass = Number of moles × Molar Mass
D
Number of moles = Molar Mass × Mass

What volume does 1 mole of any ideal gas occupy at STP (Standard Temperature and Pressure)?

A
22.7 L
B
22.4 L
C
23.7 L
D
24.5 L

Which equation is used for calculating the volume of gas when not at STP?

A
PV = nRT
B
P = V × n × R × T
C
V = n × P × T
D
PV = n × R × T

What is the limiting reactant in a chemical reaction?

A
The reactant that is present in excess
B
The reactant that is completely consumed first
C
The reactant that determines the temperature of the reaction
D
The reactant that determines the color of the product

The theoretical yield of a chemical reaction is the:

A
Amount of product obtained in an experiment
B
Maximum amount of product that could be formed
C
Amount of reactant required for the reaction
D
Amount of excess reactant left over

What does the percentage yield of a reaction indicate?

A
The ratio of actual yield to theoretical yield
B
The amount of reactant used in the reaction
C
The amount of excess reactant left over
D
The efficiency of the reaction process

Which of the following steps is essential when determining the empirical formula of a compound?

A
Convert the mass of each element to moles
B
Divide the moles by the mass of each element
C
Add up the total mass of each element
D
Use the molar volume for gases

What is the empirical formula for a compound containing 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen?

A
C₂H₆O
B
CH₂O
C
C₆H₁₂O₆
D
C₁H₂O₁

How is the molecular formula determined once the empirical formula is known?

A
By dividing the molar mass by the empirical formula mass
B
By calculating the density of the solution
C
By multiplying the empirical formula by the molar mass
D
By finding the volume of the solution

What is the molar mass of water (H₂O)?

A
16.00 g/mol
B
18.02 g/mol
C
20.00 g/mol
D
14.02 g/mol

What is the primary purpose of a back titration?

A
To measure the volume of the solution
B
To determine the concentration of a substance indirectly
C
To create a standard solution
D
To measure the mass of the solute

What is the ideal gas law equation?

A
PV = nRT
B
PV = mRT
C
V = nRT
D
P = nVRT

In a titration, what does the equivalence point signify?

A
The point where the reactants are present in excess
B
The point where the reaction is complete
C
The point where no more reactant is added
D
The point where the analyte is still in excess

What is the formula for molarity?

A
Molarity = Moles of solute / Volume of solution
B
Molarity = Volume of solution / Moles of solute
C
Molarity = Moles of solvent / Volume of solute
D
Molarity = Moles of solute × Volume of solution

What is the definition of ppm (parts per million)?

A
1 mg of solute per L of solution
B
1 g of solute per 1 L of solution
C
1 mol of solute per L of solution
D
1 g of solute per kg of solution

In a titration calculation, how do you calculate the concentration of the unknown solution?

A
Using the volume and molarity of the titrant
B
Using the volume of the analyte and the molarity of the titrant
C
Using the mass of the analyte and the volume of titrant
D
Using the temperature and pressure of the solution

How is the molecular formula derived from the empirical formula?

A
By multiplying the empirical formula by the molar mass
B
By dividing the empirical formula mass by the molar mass
C
By multiplying the empirical formula by an integer 'n'
D
By calculating the number of atoms in the empirical formula

Which of the following best describes the role of an indicator in a titration?

A
To increase the volume of the titrant
B
To change color at the equivalence point
C
To ensure the solution is acidic
D
To maintain the pH of the solution

What happens during a back titration?

A
A known excess of a reactant is added to the analyte
B
The analyte is directly titrated with the titrant
C
The analyte is reacted with a known volume of solvent
D
A known excess of an indicator is used

Which of the following is a valid assumption for the Beer-Lambert Law?

A
The absorbing species should not fluoresce or phosphoresce
B
The solution can be concentrated
C
The path length of the light can vary with the concentration
D
The solution must scatter light

What does the Beer-Lambert Law equation A = εbc represent?

A
Absorbance is related to concentration and path length
B
Absorbance is proportional to temperature and pressure
C
Absorbance is equal to the concentration of the solution
D
Absorbance is related to the volume of solution

What is the purpose of the calibration curve in spectrophotometry?

A
To determine the molar absorptivity of the substance
B
To calculate the concentration of the analyte in unknown samples
C
To determine the path length of the light
D
To calculate the absorbance of a solution

What is the primary application of spectrophotometry in analytical chemistry?

A
Monitoring the rate of a chemical reaction
B
Determining the concentration of an unknown solution
C
Determining the temperature of a solution
D
Measuring the pH of a solution

Which of the following is true for an ideal gas at STP?

A
1 mole of gas occupies 22.7 L
B
1 mole of gas occupies 1 L
C
The volume of gas is proportional to the temperature in Kelvin
D
The volume of gas is inversely proportional to the pressure

What is the main difference between empirical and molecular formulas?

A
Empirical formulas represent the actual number of atoms in a compound
B
Molecular formulas represent the simplest whole-number ratio of elements in a compound
C
Empirical formulas represent the simplest whole-number ratio of elements in a compound
D
Molecular formulas represent the amount of solute in a solution

What is the most commonly used unit of concentration for liquid solutions?

A
Molarity
B
Parts per million
C
Volume percent
D
Mass percent

What is the main assumption for using the Beer-Lambert law?

A
The solution must be highly concentrated
B
The absorbing species should not interact with the solvent
C
The absorbing species must be at low temperature
D
The path length should be variable