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CC14H SC18H
Pearson GCSE Combined and Separate Chemistry Higher
Question | Answer |
---|---|
Define the rate of a reaction. | The rate at which reactants are used up or products are made. |
Describe or sketch a reactants vs time graph | Starts high and curves downward, decreasing rapidly at first and then more gently. |
Describe or sketch a products vs time graph | Starts low and curves upwards, increasing rapidly at first and then more gently. |
Explain two of the three ways the rate of a reaction that produces a gas can be measured. | Collect gas in a gas syringe and measure the volume every 30 secs/ Collect gas over water (up-turned measuring cylinder full of water) and measure volume every 30 secs/ Do reaction on a balance and record the change in mass every 30 secs. |
Explain how the rate of a reaction that goes cloudy can be measured. | Do the reaction in a beaker placed on piece of paper with a cross marked on it. Looking down through the beaker, time how it takes for the cross to disappear. |
What are the two statements of the collision theory of reactions? | States that for two particles to react they must: Collide with each other / Collide with enough energy to react |
Define the activation energy of a chemical reaction. | The minimum energy that two particles must have when they collide in order to react. |
Explain the effect of increasing the concentration on the rate of a reaction in terms of collision theory | Increasing the concentration increases the rate because there are more particles so there are more collisions and more reactions. |
Explain the effect of increasing the surface area on the rate of a reaction in terms of collision theory | Increasing the surface area (by decreasing particle sizes) increases the rate by exposing more particles to collisions leading to more collisions and more reactions. |
Explain the effect of increasing the pressure on the rate of a reaction in terms of collision theory | Increasing the pressure increases the rate because particles are pushed closer together so they collide more often |
Explain the effect of increasing the temperature on the rate of a reaction in terms of collision theory | Increasing the temperature increases the rate because particles move faster so they collide more, and collide with more energy to a greater proportion of collisions lead to reactions. |
What is a catalyst? | A substance that speeds up a chemical reaction without being used up. |
Explain the effect of a catalyst on the rate of the reaction. | Catalysts increase the rate of reaction by reducing the activation energy so that a greater proportion of collisions lead to reactions. |
What is the rate of a chemical reaction in terms of reactants? | How quickly the reactants in a reaction are used up |
What is the rate of a chemical reaction in terms of products? | How quickly the products in a reaction are formed |
What is the formula for a mean rate of reaction in terms of reactants? | quantity of reactant used/time taken |
What is the formula for a mean rate of reaction in terms of products? | quantity of reactant product formed/time taken |
How can you measure the quantity of a reactant or product? | In grams or in cm³ |
What are the two possible units for rate of reaction? | g/s or cm³/s (where s is seconds) |
How could you measure the rate of a reaction from a graph? | Draw a tangent to the curve and calculate the gradient. |
What is "collision theory"? | The theory that chemical reactions only occur when particles collide with sufficient energy |
What factors can affect the rate of a reaction? | Temperature, surface area of a solid, concentration or reactants in solution, pressure of gases |
State the effect of increasing the surface area on the rate of a reaction | Increases the rate |
Explain why increasing the surface area increases the rate of a reaction | More particles are available to collide, there are therefore more frequent collisions between reactants. |
State the effect of increasing the concentration on the rate of reaction | Increases |
Explain why increasing the concentration increases the rate of reaction | More concentrated means more particles in solution, therefore more frequent collisions between reactants. |
State the effect on increasing the pressure of a gas on the rate of reaction | Increases |
Explain why increasing the pressure of a gas increases the rate of a reaction | Less space for the particles to move around in, therefore more frequent collisions |
State the effect of increasing the temperature on the rate of reaction | Increases |
What is the activation energy? | The amount of energy a particle needs before it will be able to react when it collides with another particle |
Explain why increasing the temperature increases the rate of reaction | Increases the speed at which particles move therefore more frequent collisions. Increases the number of particles which have the activation energy therefore more collisions result in a reaction. |
What is a catalyst? | Something which changes the rate of a reaction but is not used up in that reaction |
What supplies the enzyme for producing alcoholic drinks | Yeast |