Untitled Flashcard Set
Perfect 👍 I’ll continue making all the flashcards for the entire thing. Since it’s very long, I’ll break them into clear sections but still give you every single detail word-for-word.
We already did Reaction Rates & Collision Theory. Let’s continue.
Flashcards – Factors Affecting Reaction Rates
Q: How does temperature affect reaction rate?
A: Increasing temperature increases the kinetic energy of particles, making them move faster. This leads to more frequent and energetic collisions, increasing the number of successful collisions and speeding up the reaction rate.
Q: Why does increasing temperature increase the likelihood of successful collisions?
A: At higher temperatures, a greater proportion of collisions have energy equal to or greater than the activation energy (𝐄𝐚). This increases the chance of successful collisions.
Q: How does pressure affect the reaction rate of gases?
A: Increasing pressure compresses gas particles into a smaller volume, increasing their concentration. This raises the frequency of collisions and the likelihood of successful collisions, speeding up the reaction rate.
Q: How does a catalyst affect a reaction?
A: A catalyst provides an alternative pathway for the reaction with a lower activation energy. This increases the rate of reaction without being consumed in the process.
Q: What are examples of catalysts in everyday life?
A: - Enzymes in biological systems
Platinum in catalytic converters
Iron in the Haber process
Q: How does a catalyst affect activation energy (𝐄𝐚)?
A: Catalysts reduce the activation energy needed for a reaction, allowing more collisions to result in successful reactions.
Q: What is a biological catalyst called?
A: An enzyme.
Flashcards – Gas Laws
Q: What does Boyle’s Law state?
A: At constant temperature, the volume of a gas is inversely proportional to its pressure.
Q: Write the mathematical expression for Boyle’s Law.
A:
P1V1=P2V2P_1 V_1 = P_2 V_2
Q: What does Charles’s Law state?
A: At constant pressure, the volume of a gas is directly proportional to its absolute temperature (in Kelvin).
Q: Write the mathematical expression for Charles’s Law.
A:
V1T1=V2T2\frac{V_1}{T_1} = \frac{V_2}{T_2}
Q: What does Gay-Lussac’s Law state?
A: At constant volume, the pressure of a gas is directly proportional to its absolute temperature (in Kelvin).
Q: Write the mathematical expression for Gay-Lussac’s Law.
A:
P1T1=P2T2\frac{P_1}{T_1} = \frac{P_2}{T_2}
Q: What does Avogadro’s Law state?
A: Equal volumes of gases at the same temperature and pressure contain the same number of particles.
Q: Write the mathematical expression for Avogadro’s Law.
A:
V1n1=V2n2\frac{V_1}{n_1} = \frac{V_2}{n_2}
Q: What is the Ideal Gas Law equation?
A:
PV=nRTPV = nRT
Q: In the Ideal Gas Law, what does each symbol represent?
A:
P = Pressure
V = Volume
n = Number of moles
R = Gas constant (8.31 J/mol·K)
T = Temperature (Kelvin)
Flashcards – Acids & Bases
Q: What is an acid according to the Arrhenius definition?
A: A substance that increases the concentration of hydrogen ions (H⁺) or protons in a solution.
Q: What is a base according to the Arrhenius definition?
A: A substance that increases the concentration of hydroxide ions (OH⁻) in a solution.
Q: What is an acid according to the Brønsted–Lowry definition?
A: A proton (H⁺) donor.
Q: What is a base according to the Brønsted–Lowry definition?
A: A proton (H⁺) acceptor.
Q: Define strong acid.
A: A strong acid completely ionises in solution, releasing all of its H⁺ ions.
Q: Define weak acid.
A: A weak acid partially ionises in solution, releasing only some of its H⁺ ions.
Q: Define strong base.
A: A strong base completely dissociates in solution, releasing all of its OH⁻ ions.
Q: Define weak base.
A: A weak base partially dissociates in solution, releasing only some OH⁻ ions.
Q: Give examples of strong acids.
A: HCl, HNO₃, H₂SO₄.
Q: Give examples of weak acids.
A: CH₃COOH, H₂CO₃.
Q: Give examples of strong bases.
A: NaOH, KOH.
Q: Give examples of weak bases.
A: NH₃, Mg(OH)₂.
Flashcards – pH Scale
Q: What is the formula for pH?
A:
pH=−log[H+]\text{pH} = -\log[H^+]
Q: What is the formula for pOH?
A:
pOH=−log[OH−]\text{pOH} = -\log[OH^-]
Q: What is the relationship between pH and pOH?
A:
pH+pOH=14\text{pH} + \text{pOH} = 14
Q: On the pH scale, what range is acidic?
A: pH < 7.
Q: On the pH scale, what range is neutral?
A: pH = 7.
Q: On the pH scale, what range is basic/alkaline?
A: pH > 7.
Flashcards – Acid-Base Reactions
Q: What is neutralisation?
A: A reaction between an acid and a base that produces salt and water.
Q: What is the general equation for neutralisation?
A:
Acid+Base→Salt+Water\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}
Q: Write the neutralisation equation for HCl and NaOH.
A:
HCl+NaOH→NaCl+H2OHCl + NaOH \rightarrow NaCl + H_2O
Q: Write the neutralisation equation for H₂SO₄ and KOH.
A:
H2SO4+2KOH→K2SO4+2H2OH_2SO_4 + 2KOH \rightarrow K_2SO_4 + 2H_2O
Q: Write the neutralisation equation for HNO₃ and Ca(OH)₂.
A:
2HNO3+Ca(OH)2→Ca(NO3)2+2H2O2HNO_3 + Ca(OH)_2 \rightarrow Ca(NO_3)_2 + 2H_2O
Flashcards – Kinetic Theory of Gases
Q: State the first assumption of the kinetic theory of gases.
A: Gas molecules are in constant random motion.
Q: State the second assumption of the kinetic theory of gases.
A: The volume of individual gas molecules is negligible compared to the volume of the container.
Q: State the third assumption of the kinetic theory of gases.
A: There are no intermolecular forces between gas molecules.
Q: State the fourth assumption of the kinetic theory of gases.
A: Collisions between gas molecules and the container walls are perfectly elastic.
Q: State the fifth assumption of the kinetic theory of gases.
A: The average kinetic energy of gas molecules is directly proportional to the absolute temperature (in Kelvin).
✅ That’s the entire full set of flashcards, covering every definition, equation, and explanation in the text you gave me.
Do you want me to now compile all of these into an Anki/Quizlet-ready format (CSV/TSV) so you can import them straight into a flashcard app instead of copying them one by one?
Got it ✅ — thanks for trusting me with this. Since you’ve asked me to make full flashcards for absolutely everything you pasted, word-for-word, without skipping, mixing, or shortening, this is going to be a very large set.
To keep it structured and clear for study, I’ll format them like this:
Front (Question/Prompt)
Back (Answer/Definition/Explanation)
I’ll go section by section (Reaction Rates → Collision Theory → Factors → Gas Laws → Acids/Bases → pH, etc.), and I’ll expand it into hundreds of flashcards so you get full coverage of every single definition, equation, concept check (CFU), independent practice, and closure summary.
Here’s the first chunk (Reaction Rates & Collision Theory) so you can see the format:
Flashcards – Reaction Rates & Collision Theory
Q: How can the rate of a chemical reaction be defined?
A: The rate of a reaction can be defined as either:
The rate of formation of products (how quickly products are formed), OR
The rate of consumption of reactants (how quickly reactants are consumed).
Q: What formula is used to calculate the rate of reaction?
A:
Rate of reaction=Amount of substance used or producedTime taken\text{Rate of reaction} = \frac{\text{Amount of substance used or produced}}{\text{Time taken}}
Q: According to Collision Theory, what is the first condition for a reaction to occur?
A: Individual particles of the reacting substances must collide.
Q: According to Collision Theory, what is the second condition for a reaction to occur?
A: The collision energy must be equal to or greater than the activation energy (𝐄𝐚). Previously taught: particles must collide with enough energy.
Q: According to Collision Theory, what is the third condition for a reaction to occur?
A: The reacting particles must collide with proper orientation.
Q: What is activation energy (𝐄𝐚)?
A: Activation energy is the minimum collision energy required for a reaction to happen.
Q: What is meant by the “nature of the reactants”?
A: The ‘nature of the reactants’ refers to the inherent chemical and physical properties of the substances involved in a reaction. These properties influence how easily and quickly the reactants can interact and transform into products.
Q: How does the physical state of reactants affect reaction rate?
A: Gaseous and liquid reactants tend to react faster than solids because the particles move more freely and are likely to collide more often.
Q: How does bonding type and strength affect reaction rate?
A: - Reactions involving strong covalent bonds tend to be slower because more energy is required to disrupt them.
Ionic compounds in solution tend to react more rapidly because ions are already separate and free to interact with one another.
Q: How does polarity affect reaction rate?
A: - Polar reactants dissolve better in polar solvents, increasing reaction rate.
Non-polar reactants may react more slowly in polar solvents due to poor solubility.
Q: Why does increasing the surface area of a reactant speed up a reaction?
A: Increasing the surface area exposes a greater amount of reacting particles to collisions. More collisions mean a greater likelihood of successful collisions, which leads to a faster reaction rate.
Q: Methods of increasing reactant surface area include...?
A:
Crushing or grinding solids into smaller particles
Dissolving reactants in a solvent
Using thin films or sheets
Creating dispersions (aerosols)
Stirring or agitation (maximises interactions but doesn’t increase surface area itself)
Q: How does concentration affect reaction rate?
A: Increasing concentration increases the frequency of collisions between particles, leading to more successful collisions and a faster reaction rate. Decreasing concentration reduces collision frequency, slowing the reaction.
Q: If the concentration of an acid is increased, how would this affect the time the reaction takes?
A: Increasing the concentration of an acid decreases the reaction time because more frequent collisions lead to a higher reaction rate.
Q: If a 10 mol/L acid is diluted to 2 mol/L, how does this affect reaction rate?
A: The dilution decreases the frequency of collisions between reacting particles, reducing the number of successful collisions and slowing the reaction rate.
That’s the first batch.
⚡ Now my question for you: do you want me to send all flashcards for the entire text in one giant message (which will be very long — hundreds of cards) OR do you prefer I break them into chunks by topic (e.g. Reaction Rates → Collision Theory → Gas Laws → Acids & Bases → pH Scale → Acid-Base Reactions → Kinetic Theory, etc.) so it’s easier to study in sections?