Paper 2

• What is the focus of the video discussed?

  AQA GCSE chemistry paper 2
• What does the rate of reaction indicate?

  How quickly reactants are used or products made
• How can the mean rate of reaction be calculated?

  Quantity of reactant used divided by time
• What are the units for measuring the rate of reaction?

  Grams per second, cm³ per second, moles per second
• What does a steep curve on a reaction graph indicate?

  A high rate of reaction
• What is the purpose of a stopwatch in reaction rate experiments?

  To measure the time taken for reactions
• How do you measure the change in mass in a reaction?

  Using a balance and recording at intervals
• Why do we use cotton wool in the conical flask during mass measurement?

  To allow gases to escape without losing substances
• How is the rate of reaction calculated using mass change?

  Rate = change in mass divided by change in time
• What is the method for measuring gas volume produced?

  Using a gas syringe or measuring cylinder
• How do you calculate the mean rate of reaction from a graph?

  Change in amount divided by change in time
• What does a tangent on a reaction graph represent?

  The rate of reaction at a specific point
• What is Collision Theory?

  It explains how factors affect reaction rates
• What is activation energy?

  The minimum energy needed for a reaction
• How does increasing temperature affect reaction rates?

  Increases energy and frequency of collisions
• What happens to reaction rates when pressure increases?

  Particles become more crowded, increasing collisions
• How does concentration affect reaction rates?

  Higher concentration leads to more frequent collisions
• What is the effect of increasing surface area on reaction rates?

  Increases the number of exposed reactant particles
• What is a catalyst?

  A substance that speeds up reactions without being used
• How do catalysts affect activation energy?

  They provide a lower activation energy pathway
• What is a reversible reaction?

  Products can react to form original reactants
• What is equilibrium in a reversible reaction?

  Forward and backward reactions occur at the same rate
• What factors can change the position of equilibrium?

  Concentration, temperature, and pressure changes
• What is the effect of adding a catalyst on equilibrium?

  No effect on the position of equilibrium
• What happens to hydrated copper sulfate when heated?

  It breaks down to anhydrous copper sulfate and water
• What color change occurs when hydrated copper sulfate is heated?

  Changes from blue to white
• What is the relationship between endothermic and exothermic reactions in reversible processes?

  Endothermic in one direction, exothermic in the other
• What is the significance of energy transfer in reversible reactions?

  Equal amounts of energy are transferred in both directions
• What is the color of anhydrous copper sulfate?

  White
• What happens to the color of anhydrous copper sulfate when water is added?

  It turns blue when hydrated
• How does the position of equilibrium relate to industrial processes?

  Changing conditions can optimize product yield
• What is meant by equilibrium in a reversible reaction?

  Forward and backward reactions occur at the same rate
• Under what condition do we have equilibrium in a reversible reaction?

  In a closed system with no escape of reactants or products
• What factors can control the position of equilibrium?

  Concentration, temperature, and pressure changes
• What effect does adding a catalyst have on equilibrium?

  It speeds up the rate of reaction without changing equilibrium
• What does Le Chatelier's principle state?

  A system at equilibrium will adjust to counteract changes
• What happens to equilibrium when the concentration of a substance is increased?

  Equilibrium shifts to the opposite side to reduce it
• In the Haber process, what happens if the concentration of nitrogen is increased?

  Equilibrium shifts to the right to produce more ammonia
• How does temperature affect the position of equilibrium?

  Equilibrium shifts to minimize temperature changes
• What happens to equilibrium if the forward reaction is exothermic and temperature is increased?

  Equilibrium shifts to the endothermic side