Stoichiometry Quick Fire

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A fast true/false quiz on stoichiometry concepts.

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Havana Rooseleer

United Arab Emirates

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1	Havana Rooseleer December 3, 2025	% 88	02:27

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Stoichiometry Quick Fire


Stoichiometry Quick FireOnline version A fast true/false quiz on stoichiometry concepts. by Havana Rooseleer 1 One mole contains 6.02 x 10^23 particles, a value known as Avogadro's number. Yes No 2 The number of moles from mass is calculated as n = mass / Mr (molar/formula mass). Yes No 3 Moles cannot be calculated from information about elementary entities, only from mass. Yes No 4 Avogadro’s number is 6.02 × 10^21, not 10^23. Yes No 5 The formula mass is always measured in kilograms per mole. Yes No 6 In the burger analogy, the limiting reagent is the ingredient you have the most of. Yes No 7 H2 + C -> CH4 is a reaction where oxygen is produced as a product. Yes No 8 In the methane formation example, carbon is the limiting reagent when 10.0 g H2 reacts with 5.00 g C to form CH4. Yes No 9 One mole of any substance always contains exactly 1000 molecules. Yes No 10 The volume method can determine the limiting reagent for all gas reactions, regardless of conditions. Yes No 11 Hydrogen is the limiting reagent when 0.38 g H2 reacts with 3.20 g O2. Yes No 12 If you know the mass and the volume of a solution, you cannot determine its concentration. Yes No 13 In the reaction between 10.0 g Na and 10.0 g Cl2, chlorine is in excess. Yes No 14 Oxygen is the limiting reagent when 1 g carbon reacts with 1 g oxygen to form CO2. Yes No 15 To find moles from concentration and volume, use n = C × V (with V in liters). Yes No 16 Molar mass for elements equals the atomic mass on the periodic table, while for compounds it equals the formula mass. Yes No 17 To convert between moles and particles, multiply moles by Avogadro’s number: N = n × Na. Yes No

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Stoichiometry Quick Fire

Yes or No

About this activity

Created by

Download the paper version to play

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Yes or No

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Yes or No

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Stoichiometry Quick FireOnline version

by Havana Rooseleer

One mole contains 6.02 x 10^23 particles, a value known as Avogadro's number.

The number of moles from mass is calculated as n = mass / Mr (molar/formula mass).

Moles cannot be calculated from information about elementary entities, only from mass.

Avogadro’s number is 6.02 × 10^21, not 10^23.

The formula mass is always measured in kilograms per mole.

In the burger analogy, the limiting reagent is the ingredient you have the most of.

H2 + C -> CH4 is a reaction where oxygen is produced as a product.

In the methane formation example, carbon is the limiting reagent when 10.0 g H2 reacts with 5.00 g C to form CH4.

One mole of any substance always contains exactly 1000 molecules.

The volume method can determine the limiting reagent for all gas reactions, regardless of conditions.

Hydrogen is the limiting reagent when 0.38 g H2 reacts with 3.20 g O2.

If you know the mass and the volume of a solution, you cannot determine its concentration.

In the reaction between 10.0 g Na and 10.0 g Cl2, chlorine is in excess.

Oxygen is the limiting reagent when 1 g carbon reacts with 1 g oxygen to form CO2.

To find moles from concentration and volume, use n = C × V (with V in liters).

Molar mass for elements equals the atomic mass on the periodic table, while for compounds it equals the formula mass.

To convert between moles and particles, multiply moles by Avogadro’s number: N = n × Na.