WorksheetsWeek 1 and 2 final part 2
Total questions: 20
Worksheet time: 10mins
Charles’s Law relates volume and:
Pressure
Temperature
Moles only
Density
A heated balloon expands mainly because:
Moles decrease
Temperature increases volume
Pressure increases and volume decreases
Density increases
Dalton’s Law applies best to:
A single pure gas
A mixture of gases
A solid and liquid mixture
Only oxygen gas
Partial pressure is the pressure contributed by:
The container
One gas in a mixture
The liquid in the container
The temperature
Graham’s Law explains that diffusion rate is related to:
Temperature only
Molar mass
Atomic number
pH
Lighter gases diffuse faster because they:
Have stronger bonds
Move faster at the same temperature
Have more shells
Have higher melting points
Balanced equations reflect conservation of:
Temperature
Mass
Volume
Charge only
Balancing an equation changes:
Subscripts
Coefficients
Element identities
Atomic numbers
Changing a subscript in H₂O would:
Balance the equation
Change the substance
Keep atoms conserved
Increase reaction rate
A mole is a:
Volume unit
Counting unit
Temperature unit
Pressure unit
Avogadro’s number is used to convert between:
Temperature and pressure
Particles and moles
Mass and volume only
Heat and work
Stoichiometry primarily uses:
Color change
Mole ratios from balanced equations
Atomic radius trends
pH indicators
Molar mass is commonly used to convert between:
Moles and grams
pH and concentration
Pressure and volume
Entropy and ΔG
The coefficients in a balanced equation represent:
Atom sizes
Mole ratios
Electron shells
Bond energies only
In a reaction, the limiting reactant is the one that:
Has the highest molar mass
Runs out first
Is always a gas
Has the most atoms
If the limiting reactant is used up, the reaction:
Continues indefinitely
Stops producing more product
Becomes nuclear
Increases entropy automatically
A + B → AB is:
Decomposition
Synthesis
Double replacement
Combustion
AB → A + B is:
Synthesis
Decomposition
Combustion
Neutralization
Hydrocarbon + O₂ → CO₂ + H₂O is:
Single replacement
Combustion
Double replacement
Decomposition
Single replacement reactions involve:
Two compounds swapping ions
One element replacing another in a compound
Splitting one compound
Burning oxygen only
