Stoichiometry-Test-1

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Question 1:

What is the empirical formula of a compound formed by elements X and Y, given that the percentage of X is 20% (At.wt=40) and that of Y is 80% (At.wt=80)?

A) XY²
B) X²Y
C) XY
D) XY³

Topic: Empirical Formula Determination

Correct Answer: A) XY²

Detailed Hints:

When determining the empirical formula of a compound, we must consider the mass percentage and atomic weights of the elements that constitute the compound.
In a 100g sample of this compound, there are 20g of X and 80g of Y.
We calculate the number of moles for elements X and Y. For X, we have 20g/40 (at. wt) = 0.5 moles; for Y, we have 80g/80 (at. wt) = 1 mole.
The ratio of X: Y is calculated as 0.5 moles: 1 mole, which simplifies to 1: 2.
Thus, the empirical formula for the compound is XY², which corresponds to option A.

Question 2:

What principle allows us to determine the volume of another substance if we know the mass of one substance, by using a chemical equation?

A) Mass-mass relationship
B) Mass-mole relationship
C) Mass-volume relationship
D) Mole-volume relationship

Topic: Stoichiometric Calculations

Correct Answer: C) Mass-volume relationship

Detailed Hints:

Stoichiometry is a branch of chemistry that deals with the numerical relationships of elements and compounds, and the mathematical proportions of reactants and products in chemical reactions.
As specified in option C, a mass-volume relationship is a crucial principle in stoichiometry. This relationship allows us to determine the volume of one substance (typically a gas) if the mass of another substance is known, and vice versa.
This is possible because 1 mole of any gas at standard temperature and pressure (273 K and 1 atm) occupies a volume of 22.4 L.

Question 3:

How many molecules are approximately present in 4.25 g of NH₃?

A) 1.0 × 10²³
B) 1.5 × 10²³
C) 2.0 × 10²³
D) 6.0 × 10²³

Topic: Mole-Molecule Calculations

Correct Answer: B) 1.5 × 10²³

Detailed Hints:

In chemistry, we often need to translate between the mass of a substance and the number of entities (atoms, molecules, etc.) it contains. This is done using the mole concept.
The number of moles of ammonia (NH₃) is calculated by dividing the mass by its molar mass (4.25 g / 17 g/mol = 0.25 mol).
The number of molecules can then be determined using Avogadro’s number (6.023 × 10²³), as the number of molecules in 0.25 mole of ammonia = 0.25 × 6.023 × 10²³ = 1.5 × 10²³, corresponding to option B.

Question 4:

What is the percent by mass of nitrogen in nicotine, if its molecular formula is C₁₀H₁₄N₂ and its molar mass is 162 g?

A) 4.8 %
B) 8.6 %
C) 17.2 %
D) 21.8 %

Topic: Percent Composition Calculations

Correct Answer: C) 17.2 %

Detailed Hints:

The percent composition of an element in a compound can be calculated by dividing the total mass of the element in the formula by the molar mass of the compound and multiplying by 100%.
The molar mass of nitrogen (N) is 14, so for two nitrogen atoms (N₂), it would be 28.
Therefore, the mass percentage of nitrogen in nicotine = (mass of Nitrogen / molar mass of nicotine) * 100%, which gives 28/162 * 100% = 17.2%. Thus, option C is the correct answer.

Question 5:

A compound weighing 0.8g is burned, resulting in the release of 0.2g of carbon dioxide. How many gram atoms of Carbon does the compound contain?

A) 6.8 g
B) 4.3 g
C) 0.56 g
D) 2.7 g

Topic: Atom Calculations in Combustion

Correct Answer: C) 0.56 g

Detailed Hints:

To find the number of gram atoms of Carbon in the compound, first determine the percentage composition of Carbon.
This is done by multiplying the ratio of carbon dioxide produced to compound burned by the ratio of the molar mass of Carbon to the molar mass of carbon dioxide, and then multiplying by 100: (0.2/0.8) * (12/44) * 100 = 6.8%.
The number of gram atoms is then found by dividing this percentage by the molar mass of Carbon: 6.8/12 = 0.56 g.

Question 6:

What is the weight in grams of 0.02 moles of magnesium sulfate (MgSO₄), given its molar mass is 120 g/mol?

A) 0.12 g
B) 0.24 g
C) 1.2 g
D) 2.4 g

Topic: Mole-Mass Calculations

Correct Answer: D) 2.4 g

Detailed Hints:

To determine the mass of a given number of moles of a compound, we multiply the number of moles by the molar mass of the compound.
In this case, the mass of magnesium sulfate is found by multiplying the number of moles (0.02) by the molar mass (120 g/mol): 0.02 * 120 = 2.4 g.

Question 7:

Given that two moles of hydrogen (H₂) and two moles of oxygen (O₂) react to form water (H₂O), which is the limiting reactant?

A) Hydrogen
B) Oxygen
C) None of them
D) Both of them

Topic: Limiting Reactant Calculations

Correct Answer: A) Hydrogen

Detailed Hints:

The limiting reactant in a chemical reaction is the reactant that is completely consumed first and therefore determines the maximum amount of product that can be formed.
In the formation of water, the balanced chemical equation 2H₂ + O₂ → 2H₂O shows that two moles of hydrogen react with one mole of oxygen.
Therefore, given two moles of both hydrogen and oxygen, hydrogen would run out first and is hence the limiting reactant.

Question 8:

Which of the following substances contains the highest number of oxygen atoms?

A) 2g of CO
B) 2g of N₂O
C) 2g of H₂O
D) All have an equal number of oxygen atoms.

Topic: Oxygen Atom Counting in Molecules

Correct Answer: C) 2g of H₂O

Detailed Hints:

You calculate the moles of a substance by dividing the mass by the atomic weight.
H₂O has the lowest atomic weight among all the given options, hence it will have the maximum number of moles.
The same number of moles of any substance will contain an equal number of atoms/molecules.
Therefore, H₂O contains the maximum number of oxygen atoms.

Question 9:

What volume of CO₂ is produced from the full decomposition of 126g of CaCO₃ at STP? (Atomic mass of CaCO₃ = 100).

A) 22.4 liters
B) 28.2 liters
C) 30.7 liters
D) 34.1 liters

Topic: Volume Calculation in Gas Decomposition

Correct Answer: B) 28.2 liters

Detailed Hints:

The molecular mass of calcium carbonate (CaCO₃) is 100g/mol. Hence, 126g corresponds to 1.26 moles.
The decomposition of CaCO₃ yields calcium oxide (CaO) and carbon dioxide (CO₂). The balanced chemical equation is: CaCO₃ → CaO + CO₂.
At Standard Temperature and Pressure (STP), 1 mole of a gas occupies 22.4 liters. So, 1.26 moles of CO₂ will occupy 1.26 * 22.4 = 28.224 liters.

Question 10:

An organic compound has an empirical formula of C₃H₃O. Given that the molar mass of the compound is 110.5 gmol^-1, what is the molecular formula of the compound?

A) C₃H₂O
B) C₆H₆O₂
C) C₃H₇O₃
D) C₆H₆O₃

Topic: Molecular Formula Determination

Correct Answer: B) C₆H₆O₂

Detailed Hints:

You calculate 'n' by dividing the molar mass by the mass of the empirical formula: n = 110.5 / (12 × 3 + 1.008 × 3 + 16) = 110.5 / 55.02 = 2.
An empirical formula represents the simplest whole number ratio of atoms in a compound. To get the molecular formula, multiply the empirical formula by 'n'.
Therefore, the formula is 2(C₃H₃O) = C₆H₆O₂.

Question 11:

What is the estimated quantity of molecules present in one liter of H₂O?

A) 3.35 ⨯ 10²³
B) 6.02 ⨯ 10²³
C) 3.35 ⨯ 10²⁵
D) 6.02 ⨯ 10²⁵

Topic: Quantity Estimation of Molecules in Solution

Correct Answer: C) 3.35 ⨯ 10²⁵

Detailed Hints:

One liter of water has a mass of approximately 1000 grams.
The molecular weight of water (H₂O) is 18g/mol.
Hence, the number of moles in 1 liter = mass (g) / molecular weight (g/mol), which is approximately 55.55 moles.
Multiplying the number of moles by Avogadro's number (6.02 ⨯ 10²³), yields the number of water molecules in 1 liter: 55.55 ⨯ 6.02 ⨯ 10²³ = 3.35 ⨯ 10²⁵.

Question 12:

How many atoms of chlorine are present in 2 moles of Cl?

A) 2 ⨯ 6.022⨯10²³ atoms
B) 35.5 ⨯ 6.022⨯10²³ atoms
C) 6.022⨯10²³ atoms
D) 2 ⨯ 6.022⨯10²²

Topic: Atom Counting in Moles

Correct Answer: A) 2 ⨯ 6.022⨯10²³ atoms

Detailed Hints:

The number of atoms in a mole can be calculated by multiplying the number of moles by Avogadro's number (6.022⨯10²³).
Therefore, the number of chlorine atoms in 2 moles is 2 ⨯ 6.022⨯10²³ atoms.

Question 13:

Is the empirical formula and molecular formula of a compound always the same, always different, or can it be either?

A) Always the same
B) Always different
C) Can be the same or different
D) Same only for inorganic compounds

Topic: Comparison between Empirical and Molecular Formulas

Correct Answer: C) Can be the same or different

Detailed Hints:

The molecular formula equals n times the empirical formula, where n can be any integer (1, 2, 3, and so on).
Therefore, if n equals 1, the empirical and molecular formulas are the same; otherwise, they are different.

Question 14:

What quantity of calcium oxide can be generated by heating 20 grams of calcium carbonate (CaCO₃)?

A) 5.6 grams
B) 11.2 grams
C) 22.4 grams
D) 44.8 grams

Topic: Calcium Oxide Production from Calcium Carbonate

Correct Answer: B) 11.2 grams

Detailed Hints:

In the balanced chemical equation for the decomposition of calcium carbonate (CaCO₃), it produces calcium oxide (CaO) and carbon dioxide (CO₂).
In terms of moles, 1 mole of CaCO₃ gives rise to 1 mole of CaO.
Therefore, 0.2 moles (20 g/100 g/mol) of CaCO₃ will yield 0.2 moles of CaO.
The mass of CaO thus produced can be calculated as moles x molecular weight = 0.2 moles x 56 g/mol = 11.2 grams.

Question 15:

How many molecules are present in a 22.4dm³ volume of H₂ gas at 0°C and 1 atm pressure?

A) 60.2×10²³
B) 6.02×10²³
C) 6.02×10²²
D) 6.02×10²⁵

Topic: Quantity Calculation of Molecules in a Gas

Correct Answer: B) 6.02×10²³

Detailed Hints:

According to Avogadro's law, a volume of 22.4 dm³ of any gas at 0°C and 1 atm pressure is occupied by 1 mole of the gas molecules.
This means that there are 6.022×10²³ molecules of H₂ in a 22.4 dm³ volume of H₂ gas at 0°C and 1 atm pressure.

Question 16:

In standard conditions, if air consists of 22.4% oxygen, then what is the mole count for oxygen atoms in a 1 liter air sample?

A) 0.01 moles
B) 0.02 moles
C) 0.04 moles
D) Cannot be determined

Topic: Mole Calculation of Oxygen Atoms in Air

Correct Answer: B) 0.02 moles

Detailed Hints:

22.4% of 1 liter of air means 0.224 liters of oxygen is present.
If we consider that 1 mole of any gas at standard conditions occupies 22.4 liters, then 0.224 liters of oxygen would correspond to 0.01 moles of oxygen molecules.
Each molecule of oxygen (O₂) consists of 2 atoms of oxygen. So, 0.01 moles of oxygen molecules will correspond to 0.02 moles of oxygen atoms.

Question 17:

What will be the remaining quantity of CO₂ in moles if 1021 molecules are subtracted from 200 mg of CO₂?

A) 1.66 ⨯ 10^-3
B) 2.88 ⨯ 10^-3
C) 3.35 ⨯ 10^-3
D) 4.26 ⨯ 10^-3

Topic: Calculation of Remaining Moles in CO₂

Correct Answer: B) 2.88 ⨯ 10^-3

Detailed Hints:

Begin by converting 200 mg of CO₂ to grams and then to moles using molar mass. This gives us 4.54×10^-3 moles.
Calculate the moles of 1021 molecules of CO₂ using Avogadro's number, which yields 1.66 × 10^-3 moles.
Subtract the previously calculated number of moles from the total initial moles of CO₂ to calculate the remaining moles of CO₂.

Question 18:

What is the empirical formula of an ionic compound that comprises 23g of Na, 38g of F, and 48g of O?

A) NaF₂O₂
B) NaF₂O₃
C) NaFO₃
D) NaF₃O₃

Topic: Determining the Empirical Formula of an Ionic Compound

Correct Answer: B) NaF₂O₃

Detailed Hints:

The first step is to calculate the number of moles of each component: Na, F, and O. This is done by dividing the given mass of each element by its atomic mass.
The empirical formula is then derived from the mole ratios, which in this case is NaF₂O₃.

Question 19:

Provided that the empirical formula of a compound is CH₂ and its molecular mass is 42 grams, what would be its molecular formula?

A) C₂H₄
B) C₃H₆
C) C₄H₈
D) C₅H₁₀

Topic: Calculation of Molecular Formula from Empirical Formula

Correct Answer: B) C₃H₆

Detailed Hints:

Start by calculating the molar mass of the empirical formula (CH₂), which equals 14 grams.
Then, divide the molecular mass of the compound (42 grams) by the molar mass of the empirical formula to find the integer multiple (n).
The molecular formula is then obtained by multiplying each subscript in the empirical formula by n.

Question 20:

Which of the following is responsible for the formation of non-stoichiometric compounds?

A) Only alkali metals
B) Only transition elements
C) Only noble gases
D) None of the listed

Topic: Formation of Non-Stoichiometric Compounds

Correct Answer: B) Only transition elements

Detailed Hints:

Recognize that non-stoichiometric compounds are those that do not strictly adhere to the Law of Definite Proportions.
Transition elements, with their multiple oxidation states, often form such compounds.
These compounds, such as transition metal oxides and sulfides, can deviate from idealized stoichiometry, such as FeO or FeS, exhibiting cation deficiency and variable cation-to-anion ratios.

Question 21:

If you were to completely combust 20 liters of propane, how much oxygen would you require? Consider the combustion equation:

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

A) 20 liters
B) 40 liters
C) 80 liters
D) 100 liters

Topic: Calculation of Oxygen Volume Required for Complete Combustion

Correct Answer: D) 100 liters

Detailed Hints:

Start by using the balanced equation for the combustion of propane.
It can be noted that 1 liter of propane needs 5 liters of oxygen for complete combustion.
Multiply this by the 20 liters of propane given in the question to get the total volume of oxygen required.

Question 22:

Assuming that the molar mass of oxygen is 16g/mol, how many oxygen atoms are present in 0.3 moles of ozone (O₃), which is responsible for filtering out cosmic rays from sunlight?

A) 2.01 ⨯ 10²³
B) 6.0 ⨯ 10²³
C) 3.6 ⨯ 10²³
D) 5.4 ⨯ 10²³

Topic: Determining Number of Oxygen Atoms in Ozone

Correct Answer: D) 5.4 ⨯ 10²³

Detailed Hints:

Understand that in one molecule of ozone, there are three oxygen atoms.
Therefore, in 0.3 moles of ozone, there are 0.3 * 3 = 0.9 moles of oxygen.
Multiply the moles of oxygen by Avogadro's number to get the total number of oxygen atoms.

Question 23:

When 8 grams of Hydrogen (equivalent to 4 moles) are combined with 2 moles of Oxygen, how many moles of water can be produced?

A) Three
B) Four
C) Five
D) Six

Topic: Moles of Water Produced from Hydrogen and Oxygen

Correct Answer: B) Four

Detailed Hints:

The chemical reaction between hydrogen and oxygen to form water can be represented as: 2H₂ + O₂ → 2H₂O.
However, given that 4 moles of H₂ are reacting with 2 moles of O₂, the equation becomes: 4H₂ + 2O₂ → 4H₂O.
Thus, 4 moles of water are produced.

Question 24:

Which of the following carries the smallest mass?

A) 2 grams of Nitrogen
B) A single mole of Carbon (atomic weight of Carbon is 12)
C) Half a mole of Sodium (atomic weight of Sodium is 23)
D) 4 moles of Hydrogen

Topic: Comparison of Elemental Weights

Correct Answer: A) 2 grams of Nitrogen

Detailed Hints:

Calculate the weight of 1 mole of Carbon (C) which equals 12 grams.
Calculate the weight of 1/2 mole of Sodium (Na) which equals 23/2 = 11.5 grams.
Calculate the weight of 4 moles of Hydrogen (H₂) which equals 4 * 2 = 8 grams.
The smallest mass among the given options would be 2 grams of Nitrogen.

Question 25:

If you have 5 moles of Sulphur dioxide (SO₂), what would be its mass, given that atomic mass of Sulphur (S) is 32?

A) 320 grams
B) 380 grams
C) 400 grams
D) 420 grams

Topic: Mass Calculation of Sulphur Dioxide Moles

Correct Answer: A) 320 grams

Detailed Hints:

Understand that the molecular weight of SO₂ (Sulphur dioxide) is calculated as the atomic weight of Sulphur (32) plus twice the atomic weight of Oxygen (16*2).
The molecular weight of SO₂ is therefore 32 + 16*2 = 64 grams/mole.
Multiply the molecular weight by the given number of moles (5 moles) to get the total mass: 5 * 64 = 320 grams.

Question 26:

Which statement is not true for 20 moles of H₂O?

A) They contain 40 moles of hydrogen atoms
B) They contain 20 moles of oxygen atoms
C) They contain 20 moles of hydrogen atoms
D) They encompass 120.4×10²³ molecules

Topic: Mole Relationship in Water Molecules

Correct Answer: C) They contain 20 moles of hydrogen atoms

Detailed Hints:

Recognize that one molecule of H₂O (water) consists of two hydrogen atoms and one oxygen atom.
Hence, 20 moles of water will contain twice the number of moles of hydrogen atoms, and the same number of moles of oxygen atoms.
Therefore, the correct answer is option C, as it contradicts this fact.

Question 27:

When magnesium reacts with zirconium chloride, zirconium is produced according to the following reaction:
ZrCl₄ + 2Mg → Zr + 2MgCl₂
If 0.2 moles of magnesium is used in this reaction, how many moles of zirconium would be obtained?

A) 0.01
B) 0.1
C) 0.2
D) 0.02

Topic: Mole Ratio in Chemical Reactions

Correct Answer: B) 0.1

Detailed Hints:

The balanced chemical equation reveals that two moles of magnesium react with zirconium chloride to produce one mole of zirconium.
Hence, if 0.2 moles of magnesium is used in the reaction, half of this amount (or 0.1 mole) of zirconium would be produced, given the 2:1 ratio.

Question 28:

What is the lightest element known to exist in the universe?

A) Oxygen
B) Hydrogen
C) Nitrogen
D) Silicon

Topic: Lightest Element in the Universe

Correct Answer: B) Hydrogen

Detailed Hints:

Hydrogen, with an atomic number of 1, is the first and lightest element on the periodic table.
With only one proton in its nucleus, it has the simplest atomic structure.
Therefore, hydrogen is the lightest known element in the universe.

Question 29:

To soften a 5-liter sample of hard water with a Ca2+ ion concentration of 40 mg per liter, what mass of washing soda (Na2CO3) is needed?

A) 1.2 mg
B) 5.3 mg
C) 53 mg
D) 530 mg

Topic: Water Hardness and Softening

Correct Answer: D) 530 mg

Detailed Hints:

A single liter of water holds 40mg of Ca2+, 5 liters would thus contain 40 x 5 = 200mg of Ca2+.
From the reaction, 40g of Ca2+ reacts with 106g of Na2CO3 to yield CaCO3 and 2Na+.
If 40g of Ca2+ reacts with 106g of Na2CO3, then 1g of Ca2+ should react with 106/40g of Na2CO3.
Thus, 200mg (or 200/1000g) of Ca2+ should react with (106/40) x (200/1000)g of Na2CO3, approximately 530mg.

Question 30:

What is the total number of molecules in a 9.8g sample of ice?

A) 6.02 ⨯ 10²²
B) 6.02 ⨯ 10²³
C) 3.01 ⨯ 10²³
D) 3.01 ⨯ 10²²

Topic: Molecule Calculation in a Sample

Correct Answer: C) 3.01 ⨯ 10²³

Detailed Hints:

The number of molecules in a sample can be calculated using the formula: (Mass of sample in grams / Molar mass of substance in g/mol) x Avogadro's number.
Given the molar mass of water as 18g/mol and Avogadro's number as 6.02x10²³, the number of molecules in 9.8g of ice would be (9.8/18) x 6.02x10²³.
This approximates to 3.01x10²³ molecules.

Question 31:

Given a compound consisting of 6.4 moles of X, 6.4 moles of Y, and 8.5 moles of Z, what is the empirical formula of the compound?

A) XYZ₂
B) X₂Y₂Z₃
C) X₃Y₃Z₄
D) X₄Y₄Z₅

Topic: Empirical Formula Determination

Correct Answer: C) X₃Y₃Z₄

Detailed Hints:

The empirical formula is based on the ratio of moles of each element in a compound.
For X:Y:Z, the ratio is 6.4/6.4 : 6.4/6.4 : 8.5/6.4 = 1 : 1 : 1.33.
To convert this ratio to whole numbers, multiply each term by 3, yielding a ratio of 3 : 3 : 4.
Therefore, the empirical formula of the compound is X₃Y₃Z₄.

Question 32:

Which substance contains the greatest number of molecules in a 1g sample?

A) Hydrogen
B) Carbon Dioxide
C) Oxygen
D) None of the above

Topic: Molecule Count in a Sample

Correct Answer: A) Hydrogen

Detailed Hints:

To evaluate which substance contains the most number of molecules in a 1g sample, consider the atomic mass of each element.
Hydrogen has the smallest atomic mass among the options.
The number of moles (and thus, the number of molecules) is inversely proportional to the atomic mass for a given mass of substance.
Therefore, 1g of hydrogen will contain the highest number of molecules among the given options.

Question 33:

Approximately how many atoms are there in a single molecule of Hemoglobin?

A) 5000
B) 7000
C) 10,000
D) 12,000

Topic: Atom Count in a Molecule

Correct Answer: C) 10,000

Detailed Hints:

Hemoglobin is a complex molecule and consists of a large number of atoms.
Each molecule of Hemoglobin is made of about 10,000 atoms.
This makes it significantly heavier than a hydrogen atom, by a factor of nearly 68,000 times.

Question 34:

How many moles of Mg₃(PO₄)₂ (Magnesium Phosphate) will contain 0.25 moles of Oxygen atoms?

A) 3.125 ⨯ 10^-2
B) 1.250 ⨯ 10^-2
C) 3.125 ⨯ 10^-3
D) 1.250 ⨯ 10^-3

Topic: Moles Calculation in a Compound

Correct Answer: A) 3.125 ⨯ 10^-2

Detailed Hints:

The compound Mg₃(PO₄)₂ contains 8 Oxygen atoms per molecule due to the presence of 2 PO₄ groups, each containing 4 Oxygen atoms.
Thus, 1 mole of Mg₃(PO₄)₂ contains 8 moles of Oxygen atoms.
By unitary method, if 1 mole of Mg₃(PO₄)₂ has 8 moles of Oxygen atoms, 0.25 moles of Oxygen atoms will be present in 0.25/8 moles of Mg₃(PO₄)₂, which equals 3.125 x 10^-2 moles.

Question 35:

In a 0.1g sample of Sodium, how many moles exist?

A) 4.3 × 10^-3
B) 4.3 × 10^-1
C) 4.01 × 10^-3
D) 4.3 × 10^-2

Topic: Moles Calculation in a Sample

Correct Answer: A) 4.3 × 10^-3

Detailed Hints:

The total number of moles in a given sample can be calculated by the formula: Moles = Mass of substance (in grams) / Atomic mass of substance (in g/mole).
Given the atomic mass of Sodium as 23g/mole, the number of moles in 0.1g of Sodium would be 0.1/23.
By performing the above calculation, we find that there are approximately 4.3 × 10^-3 moles of Sodium in a 0.1g sample.

Stoichiometry-Test-1

Question 1:

Topic: Empirical Formula Determination

Question 2:

Topic: Stoichiometric Calculations

Question 3:

Topic: Mole-Molecule Calculations

Question 4:

Topic: Percent Composition Calculations

Question 5:

Topic: Atom Calculations in Combustion

Question 6:

Topic: Mole-Mass Calculations

Question 7:

Topic: Limiting Reactant Calculations

Question 8:

Topic: Oxygen Atom Counting in Molecules

Question 9:

Topic: Volume Calculation in Gas Decomposition

Question 10:

Topic: Molecular Formula Determination

Question 11:

Topic: Quantity Estimation of Molecules in Solution

Question 12:

Topic: Atom Counting in Moles

Question 13:

Topic: Comparison between Empirical and Molecular Formulas

Question 14:

Topic: Calcium Oxide Production from Calcium Carbonate

Question 15:

Topic: Quantity Calculation of Molecules in a Gas

Question 16:

Topic: Mole Calculation of Oxygen Atoms in Air

Question 17:

Topic: Calculation of Remaining Moles in CO2

Question 18:

Topic: Determining the Empirical Formula of an Ionic Compound

Question 19:

Topic: Calculation of Molecular Formula from Empirical Formula

Question 20:

Topic: Formation of Non-Stoichiometric Compounds

Question 21:

Topic: Calculation of Oxygen Volume Required for Complete Combustion

Question 22:

Topic: Determining Number of Oxygen Atoms in Ozone

Question 23:

Topic: Moles of Water Produced from Hydrogen and Oxygen

Question 24:

Topic: Comparison of Elemental Weights

Question 25:

Topic: Mass Calculation of Sulphur Dioxide Moles

Question 26:

Topic: Mole Relationship in Water Molecules

Question 27:

Topic: Mole Ratio in Chemical Reactions

Question 28:

Topic: Lightest Element in the Universe

Question 29:

Topic: Water Hardness and Softening

Question 30:

Topic: Molecule Calculation in a Sample

Question 31:

Topic: Empirical Formula Determination

Question 32:

Topic: Molecule Count in a Sample

Question 33:

Topic: Atom Count in a Molecule

Question 34:

Topic: Moles Calculation in a Compound

Question 35:

Topic: Moles Calculation in a Sample

Test Results

Topic: Calculation of Remaining Moles in CO₂