18 Questions
What is the mole ratio between KCl3 and O2 in the given reaction?
2:3
How many moles of water are formed when 2 moles of hydrogen gas react with 1 mole of oxygen gas?
2 moles
If the theoretical yield of a reaction is 65 grams and the actual yield is 52 grams, what is the percent yield?
80%
Which of the following best describes the limiting reactant in a chemical reaction?
The reactant that is consumed first and limits the amount of product formed.
What is the pressure exerted by a 760 mm column of mercury at 0°C?
1 atm
According to Gay-Lussac's Law, what happens to the pressure of a gas if the temperature is decreased while the volume is held constant?
The pressure decreases.
What is the empirical formula of a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?
CH2O
For the balanced equation: $2,\ce{KClO3} \rightarrow 2,\ce{KCl} + 3,\ce{O2}$, what is the mole ratio of potassium chlorate to oxygen gas?
2:3
What is the percent composition of hydrogen in the compound $\ce{CH3CH2OH}$ (ethanol)?
13.04%
Which compound has the structural formula $\ce{CH3CH2OH}$?
Ethanol
Balance the equation: $\ce{_S8 +_O2 ->_SO3}$
$\ce{S8 + 12O2 -> 8SO3}$
For the reaction $\ce{CH4 + 2O2 -> CO2 + 2H2O}$, what is the mole ratio of methane to water?
1:2
Which type of chemical formula represents the total number of atoms of each constituent element in one molecule of a compound?
Molecular formula
In calculating the empirical formula mass, what step comes after determining the molar mass of each element in the compound?
Step 1: Calculate the Empirical Formula Mass
Which type of formula represents the ratio of the elements present in a chemical compound?
Empirical formula
What is the empirical formula of a compound if its molecular formula is C6H12O6?
CH2O
When calculating the molecular formula from the empirical formula, what is done with the subscripts found in the empirical formula?
Round off if necessary
Which represents the percentage composition of elements in a compound?
% (percentage) composition
Test your understanding of mole ratio and percent yield in chemical reactions with this quiz. Balance chemical equations and calculate the number of moles of products formed. Practice applying the concepts to solve reaction stoichiometry problems.
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