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Quizzes > Science > Chemistry

Master Chemistry Calculations - Take the Quiz!

Ready for an IGCSE chemistry calculations challenge? Dive in now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration for a free chemistry calculation quiz on a sky blue background

Calling all budding scientists and IGCSE students! Are you ready to sharpen your skills on chemistry calculation questions and answers? This interactive calculation in chemistry quiz is your ticket to mastering IGCSE chemistry calculations, from molar mass to reaction yields. In just a few minutes, you'll test your chemistry calculation practice, tackle tricky chemical calculation questions, and build unshakeable confidence. Dive into our engaging chem quiz or challenge yourself with detailed calculations with chemical formulas and equations that reinforce every concept. Jump in now and see how far your knowledge can go!

Calculate the molar mass of water (H2O).
20.03 g/mol
18.02 g/mol
17.00 g/mol
16.00 g/mol
The molar mass of H2O is found by summing two hydrogen atoms (1.01 g/mol each) and one oxygen atom (16.00 g/mol), totaling 18.02 g/mol. This calculation uses atomic masses from the periodic table. Accurate summation of constituent elements yields the correct molar mass. ChemGuide Reference
How many moles are present in 36.04 grams of water (H2O)?
4.00 mol
1.00 mol
2.00 mol
0.50 mol
Moles are calculated by dividing mass by molar mass: 36.04 g ÷ 18.02 g/mol = 2.00 mol. The molar mass of water is 18.02 g/mol. This direct conversion is fundamental in stoichiometry. Stoichiometry Text
What is the percent composition of carbon in carbon dioxide (CO2)?
16.00%
44.01%
27.29%
32.00%
Percent composition = (mass of element ÷ molar mass of compound) × 100. For carbon in CO2: (12.01 ÷ 44.01) × 100 = 27.29%. This shows the fraction of carbon by mass. Composition Guide
How many grams of NaCl are required to prepare 500 mL of a 0.20 M solution?
5.84 g
11.69 g
2.92 g
58.44 g
Moles needed = M × V = 0.20 mol/L × 0.500 L = 0.100 mol. Mass = moles × molar mass = 0.100 mol × 58.44 g/mol = 5.84 g. 58.44 g/mol is the molar mass of NaCl. Solution Prep
If 2 moles of H2 react with 1 mole of O2, how many moles of H2O are produced?
1 mol
2 mol
3 mol
4 mol
Balanced equation: 2H2 + O2 ? 2H2O. Using stoichiometry, 2 mol H2 and 1 mol O2 produce 2 mol H2O. Both reactants are completely consumed in this ratio. Stoichiometry Online
What volume does 1 mole of an ideal gas occupy at standard temperature and pressure (0°C and 1 atm)?
18.0 L
22.4 L
20.0 L
24.8 L
At STP (0°C, 1 atm), one mole of any ideal gas occupies 22.4 liters according to the Ideal Gas Law (PV=nRT). This is a standard constant in gas calculations. Ideal Gas Law
Determine the empirical formula of a compound with 40.0% C, 6.7% H, and 53.3% O by mass.
CHO
CH2O
C2H2O
C2H4O2
Assume 100 g sample: C=3.33 mol, H=6.7 mol, O=3.33 mol. Dividing by smallest (3.33) gives a ratio of 1:2:1, so the empirical formula is CH2O. Percent to moles conversion yields the ratio. Empirical Formula Tutorial
A reaction has a theoretical yield of 60.0 g but produces 50.0 g of product. What is the percent yield?
75%
120%
83.3%
16.7%
Percent yield = (actual yield ÷ theoretical yield) × 100 = (50.0 g ÷ 60.0 g) × 100 = 83.3%. It measures the efficiency of a reaction. Yield Calculations
Calculate the freezing point of a 1.00 m aqueous solution of urea (non-electrolyte). (Kf for water = 1.86 °C/m)
-0.931 °C
-1.86 °C
-3.72 °C
-0.517 °C
Freezing point depression ?Tf = i × Kf × m. For urea, i=1, so ?Tf = 1 × 1.86 °C/m × 1.00 m = 1.86 °C. The new freezing point = 0 °C - 1.86 °C = -1.86 °C. Colligative Properties
What is the pH of a buffer solution containing 0.10 M acetic acid (pKa = 4.76) and 0.10 M sodium acetate?
7.00
4.76
3.76
5.24
Using the Henderson - Hasselbalch equation: pH = pKa + log([A - ]/[HA]) = 4.76 + log(0.10/0.10) = 4.76 + 0 = 4.76. Equal concentrations yield pH equal to pKa. Buffer Equations
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Study Outcomes

  1. Understand Fundamental Mole and Mass Relationships -

    Grasp how to convert between mass, moles, and number of particles using chemistry calculation questions and answers. Build a solid foundation for tackling more complex stoichiometry problems.

  2. Apply IGCSE Chemistry Calculations to Balanced Equations -

    Use balanced chemical equations to determine reactant and product quantities accurately. Develop the skills needed for IGCSE chemistry calculations and beyond.

  3. Calculate Theoretical and Percentage Yields -

    Determine the maximum product mass and calculate percentage yield to evaluate reaction efficiency. Strengthen your ability to predict and compare experimental outcomes.

  4. Perform Solution Concentration and Dilution Calculations -

    Solve for molarity, molality, and prepare dilutions with precision. Master calculation in chemistry quiz questions involving solution chemistry.

  5. Analyze Limiting Reagents and Excess Reactants -

    Identify which reactant limits product formation and calculate leftover materials. Enhance your problem-solving approach to multi-reactant reactions.

  6. Build Confidence Through Practice -

    Tackle a variety of chemical calculation questions to reinforce concepts and self-assess progress. Boost your confidence in chemistry calculation practice for exams and quizzes.

Cheat Sheet

  1. Master the Mole Concept -

    The mole bridges atoms to grams via Avogadro's number (6.022×10^23 particles/mol). Use the formula n = mass ÷ molar mass and get comfortable moving between moles, particles, and mass for many chemistry calculation questions and answers. A quick tip: remember "Avogadro's army" to recall the huge number behind 1 mol.

  2. Precision in Molar Mass Calculations -

    Accurate relative atomic masses from sources like NIST or the Royal Society of Chemistry ensure correct molar mass values. Sum the atomic masses for compounds systematically - e.g., H₂SO₄ = 2(1.008) + 32.06 + 4(16.00) = 98.08 g/mol - and check your work. Precise molar masses are vital for reliable IGCSE chemistry calculations.

  3. Stoichiometry and Balanced Equations -

    Balanced chemical equations underpin all yield and reagent calculations in your calculation in chemistry quiz. Use mole ratios directly from coefficients to determine required or produced amounts; for instance, 2H₂ + O₂ → 2H₂O tells you 2 mol H₂ produces 2 mol H₂O. Trusted texts like Zumdahl's Chemistry emphasize practicing diverse stoichiometry problems to build speed and confidence.

  4. Empirical vs. Molecular Formulas -

    Empirical formulas show simplest whole-number ratios, while molecular formulas scale that ratio to the actual molar mass. From mass-percent data, assume 100 g of compound to find moles of each element, derive the simplest ratio, then multiply by (molar mass ÷ empirical mass) as outlined in IUPAC guidelines. A handy mnemonic: "Empirical is Essence; Molecular is More."

  5. Yield, Atom Economy, and Efficiency -

    Percentage yield = (actual yield ÷ theoretical yield) × 100%, a staple of chemistry calculation practice and essential for IGCSE chemistry calculations. For greener chemistry, calculate atom economy = (mass of desired product ÷ total mass of reactants) × 100%, as promoted by green chemistry protocols. Tracking both metrics hones your problem-solving skills and deepens understanding of sustainable processes.

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