Rate of Reactions and the Extent of Chemical change

Haber Process

An industrial process for synthesizing ammonia from nitrogen and hydrogen.

Reversible Reaction

A reaction that can proceed in both forward and reverse directions.

Ammonia (NH3)

A compound used for explosives, cleaning products, and fertilizers.

Exothermic Reaction

A reaction that releases heat, causing the temperature to rise.

Catalyst

A substance that increases the rate of a reaction without being consumed.

Compromise in Chemical Reactions

The balance between maximizing the reaction rate and achieving a high yield.

Effect of Temperature on Yield

Lower temperatures favor production yield in exothermic reactions, but slow down the reaction rate.

Effect of Pressure on Yield

Higher pressures shift equilibrium towards the products, increasing yield.

Iron Catalyst

A substance used in the Haber Process to enhance the reaction rate for ammonia synthesis.

Rate of Reaction

A measure of how fast reactants are converted into products, often measured by the change in concentration of reactants or products over time.

Collision Theory

The theory that explains how reaction rates are influenced by the frequency and energy of collisions between particles.

Factors Affecting Reaction Rate

1. Temperature: Increased temperature gives particles more energy, increasing reaction rate. 2. Concentration/Pressure: Higher concentration puts more particles in a given volume, facilitating collisions. 3. Surface Area: Greater surface area allows more particles to collide. 4. Catalysts: Substances that lower activation energy to increase reaction rate without being consumed.

Catalyst

A substance that speeds up a chemical reaction by providing an alternative pathway with a lower activation energy.

Measuring Rate of Reaction

Ways to measure reaction rate include observing color change, measuring change in mass (often of gases), and calculating the volume of gas produced using a gas syringe.

Le Chatelier's Principle

States that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

Reversible Reactions

Reactions that can proceed in both forward and reverse directions, reaching an equilibrium point where the rates of the forward and backward reactions are equal.

Endothermic Reaction

A type of reaction that absorbs heat from the surroundings.

Exothermic Reaction

A type of reaction that releases heat to the surroundings.

Equilibrium

A state in a chemical reaction where the concentrations of products and reactants remain constant over time.

Rate of reaction calc

Amount of reactant used OR amount of product formed / time

Sodium thiosulfate & HCl practical

1) measure 10 cm cubes of sodium thiosulfate

2) place flask on piece of paper with cross

3) measure 10 cm cubed of 0.1 mol/dm cubed using measuring cylinder

4) add to conical flask

5) start timer and record how long it takes for cross to no longer be visible

6) repeat with different concentrations of HCL

Magnesium and HCL practical

1) set volume of HCl in conical flask

2) add magnesium

3) plug in gas syringe

4) start 30 sec timer and record how much gas has been collected