Unlock hundreds more features
Save your Quiz to the Dashboard
View and Export Results
Use AI to Create Quizzes and Analyse Results

OR
Sign inSign in with Facebook
Sign inSign in with Google
Quizzes > Quizzes for Business > Education

Basic Chemistry and Math Assessment Quiz

Challenge Yourself with Chemistry and Math Problems

Difficulty: Moderate
Questions: 20
Learning OutcomesStudy Material
Colorful paper art representing a quiz on basic chemistry and math assessment

Dive into this engaging Basic Chemistry Knowledge Quiz combined with a Math Assessment Quiz to test your foundation in science and arithmetic. Joanna Weib invites learners, educators, and curious minds to explore core concepts in stoichiometry, algebraic problem-solving, and unit conversions. This basic chemistry and math assessment quiz is perfect for high school students sharpening their skills or anyone seeking a refresher. Customize questions and difficulty freely in our editor and tailor the experience to your needs. Ready for more? Browse other fun quizzes to continue your learning journey.

What elements are present in the compound CaCO3?
Calcium, Carbon, Oxygen
Calcium, Copper, Oxygen
Calcium, Carbon, Nitrogen
Calcium, Carbon, Hydrogen
CaCO3 consists of one calcium (Ca) atom, one carbon (C) atom, and three oxygen (O) atoms. No other elements are present in this formula.
What is the molar mass of H2O?
18.015 g/mol
16.00 g/mol
20.02 g/mol
2.02 g/mol
Water (H2O) has a molar mass of 2×1.008 (for H) + 16.00 (for O) = 18.016 g/mol, commonly rounded to 18.015 g/mol. The other values do not match this sum.
What type of reaction is represented by the equation 2H2 + O2 → 2H2O?
Synthesis
Decomposition
Single displacement
Combustion
In this reaction, hydrogen and oxygen combine to form water, which is characteristic of a synthesis reaction. Decomposition and displacement do not describe this combination process.
How many molecules are in 0.50 moles of CO2?
3.01 × 10^23 molecules
1.20 × 10^24 molecules
6.02 × 10^22 molecules
1.00 × 10^23 molecules
One mole contains 6.022×10^23 entities, so 0.50 moles × 6.022×10^23 = 3.011×10^23 molecules. The other options misapply Avogadro's number.
Convert 2500 mL to liters.
2.5 L
25 L
0.25 L
0.025 L
There are 1000 mL in 1 L, so 2500 mL ÷ 1000 = 2.5 L. The other values arise from incorrect decimal placements.
How many oxygen atoms are in one formula unit of Fe2(SO4)3?
12
7
9
6
Fe2(SO4)3 contains three sulfate ions, each with four oxygen atoms, giving 3×4 = 12 oxygens. The other counts ignore the correct ratio of sulfate groups.
What is the molar mass of NaCl?
58.44 g/mol
35.45 g/mol
22.99 g/mol
78.44 g/mol
Sodium (22.99 g/mol) plus chlorine (35.45 g/mol) equals 58.44 g/mol. The other totals are missing one element or misadded.
Identify the reaction type: Zn + 2HCl → ZnCl2 + H2.
Single replacement
Double displacement
Combustion
Synthesis
Zinc displaces hydrogen from HCl, characteristic of a single replacement reaction. No new compounds form between two reactants simultaneously, so it is not double displacement or synthesis.
What are the products when HCl reacts with NaOH?
NaCl and H2O
H2 and NaOH
NaClO and H2O
H2O2 and NaCl
Acid-base neutralization between HCl and NaOH yields salt (NaCl) and water (H2O). The other options list incorrect products for this reaction.
Calculate the molarity of a solution containing 0.25 moles of solute in 0.50 L of solution.
0.50 M
0.25 M
2.00 M
0.125 M
Molarity = moles/volume = 0.25 mol ÷ 0.50 L = 0.50 M. The other values come from incorrect division or multiplication.
A solution contains 5 g of solute in 100 g of solution. What is the mass percent of the solute?
5%
0.05%
50%
0.5%
Mass percent = (mass solute/mass solution)×100 = (5 g/100 g)×100 = 5%. The other options misplace the decimal.
How many moles are in 16.04 g of CH4?
1.00 mol
0.50 mol
2.00 mol
4.00 mol
Methane CH4 has a molar mass of 12.01 + 4×1.008 ≈ 16.04 g/mol, so 16.04 g corresponds to 1.00 mol. Other answers use incorrect division.
How much of a 1.0 M stock solution is required to prepare 100 mL of 0.20 M solution?
20 mL
200 mL
5 mL
80 mL
Use C1V1 = C2V2: (1.0 M)V1 = 0.20 M×0.100 L, so V1 = 0.020 L = 20 mL. The other volumes do not satisfy the dilution equation.
In a titration, 25.00 mL of base neutralizes 100.0 mL of 0.100 M acid. What is the base concentration?
0.40 M
0.25 M
0.10 M
0.20 M
M1V1 = M2V2 gives Mbase = (0.100 M × 0.100 L) / 0.02500 L = 0.40 M. Other answers result from incorrect arithmetic in the titration calculation.
What is the concentration in ppm of 2 mg solute dissolved in 1 L of solution?
2 ppm
0.002 ppm
2000 ppm
0.02 ppm
1 ppm corresponds to 1 mg/L, so 2 mg/L = 2 ppm. The other values come from incorrect scale factors.
A compound is 40.0% C, 6.7% H, and 53.3% O by mass. What is its empirical formula?
CH2O
C2H4O2
CHO
C2H5O
Assuming 100 g sample yields 40.0 g C (3.33 mol), 6.7 g H (6.64 mol), 53.3 g O (3.33 mol), the mole ratio is 1:2:1, giving CH2O. The others do not match this ratio.
If the theoretical yield of a reaction is 20.0 g but the actual yield is 15.0 g, what is the percent yield?
75%
133%
25%
85%
Percent yield = (actual/theoretical)×100 = (15.0 g/20.0 g)×100 = 75%. Other choices miscompute the ratio or reverse it.
In the reaction Cl2 + 2Fe2+ → 2Cl- + 2Fe3+, which species is the oxidizing agent?
Cl2
Fe2+
Cl-
Fe3+
An oxidizing agent accepts electrons; Cl2 gains electrons to become Cl-, so Cl2 is the oxidizing agent. Fe2+ is oxidized, not reduced.
A buffer contains 0.10 M HA and 0.010 M A- with pKa = 4.76. What is the pH?
3.76
4.76
5.76
2.76
Henderson - Hasselbalch: pH = pKa + log([A-]/[HA]) = 4.76 + log(0.010/0.10) = 4.76 + log(0.1) = 4.76 - 1 = 3.76. Other choices ignore the ratio term.
At STP, what volume does 2.00 moles of an ideal gas occupy?
44.8 L
22.4 L
11.2 L
89.6 L
At STP one mole of ideal gas occupies 22.4 L, so 2.00 moles occupy 2.00 × 22.4 L = 44.8 L. The others assume incorrect multiples of 22.4 L.
0
{"name":"What elements are present in the compound CaCO3?", "url":"https://www.quiz-maker.com/QPREVIEW","txt":"What elements are present in the compound CaCO3?, What is the molar mass of H2O?, What type of reaction is represented by the equation 2H2 + O2 → 2H2O?","img":"https://www.quiz-maker.com/3012/images/ogquiz.png"}

Learning Outcomes

  1. Analyse chemical formulas to determine compound composition
  2. Calculate molar masses and perform unit conversions
  3. Identify reaction types and predict reaction products
  4. Apply algebraic techniques to solve concentration problems
  5. Demonstrate arithmetic operations in chemistry contexts
  6. Evaluate data and interpret results accurately

Cheat Sheet

  1. Analyze chemical formulas - Dive into the tiny world of atoms by breaking down formulas like H₂O to reveal two hydrogen atoms and one oxygen atom. This detective work sets the stage for understanding compound composition and mastering the periodic playground. Empirical Formulae - Chemguide
  2. Calculate molar mass - Add up atomic masses to find the weight of a mole of any substance, like CO₂'s 44.01 g/mol. This skill is essential for converting between grams and moles so you can measure out reactants perfectly. Molar Mass Calculations - ChemTeam
  3. Master unit conversions - Convert grams to moles by dividing the mass by molar mass; for example, 88 g of CO₂ ÷ 44.01 g/mol gives 2 moles. Nailing these conversions lets you balance reactions and predict yields with confidence. Stoichiometry - Khan Academy
  4. Identify reaction types - Spot synthesis, decomposition, single replacement, double replacement, and combustion reactions by their unique patterns. Recognizing these families helps you predict products and write equations like a pro. Types of Chemical Reactions - Chemistry LibreTexts
  5. Solve concentration problems - Use Molarity = moles of solute ÷ liters of solution to determine how crowded your molecules are. For instance, 0.5 mol of NaCl in 2 L gives a 0.25 M solution. Molarity Calculations - ChemTeam
  6. Calculate percent composition - Crunch the numbers to see what percent of a compound's mass each element contributes, like the 11.2% hydrogen in H₂O. This arithmetic practice builds your confidence with chemical data. Percent Composition - ChemTeam
  7. Interpret data and uncertainty - Understand significant figures and measurement error to report results that are both precise and accurate. This critical skill ensures your lab reports shine and your calculations stay honest. Measurement Uncertainty, Accuracy, and Precision - Chemistry LibreTexts
  8. Identify limiting reactants - Figure out which reactant will run out first and cap your product yield, like O₂ in the reaction of H₂ with O₂ to make water. This concept is key for real-world chemistry where resources are limited. Limiting Reagent Problems - ChemTeam
  9. Balance chemical equations - Adjust coefficients so atoms are conserved, turning H₂ + O₂ → H₂O into 2H₂ + O₂ → 2H₂O. Mastering this law of conservation of mass ensures your reactions obey nature's bookkeeping. Balancing Chemical Equations - Khan Academy
  10. Learn common polyatomic ions - Memorize ions like sulfate (SO₄²❻) and nitrate (NO₃❻) to write formulas and predict reaction behavior. This cheat-sheet knowledge turns complex equations into simple puzzles. Polyatomic Ions - Chemistry LibreTexts
Make a Quiz (FREE) Copy & Edit This Quiz Create a Quiz with AI

Education Quizzes

Powered by: Quiz Maker