How to make up the different concentrations of hydrochloric acid.
Apparatus
Conical flask
6 beakers
Clamp stand
Burette
Stop clocks
Sodium Thiosulphate
Different concentrations of HCI acid.
Table 2
What is a reaction?
A reaction occurs when two reactants successfully react together to form a new product. This is called the collision theory. There is many different ways to measure the rate of reaction.
- These include: Measuring the amount of gas produced
- Weighing before and after the experiment
- Draw an X on a piece of paper and measure how long it takes for the substance to turn cloudy enough so that the X is no longer visible
- Using sensors to detect the loss of the starting material or the formation of the product
Variables:
Temperature:
If the temperature is high, the particles have more energy. As a result of them having more energy they move a lot faster. Therefore the particles collide a lot faster increasing the rate of reaction and making a new product.
Examples of reactions:
An example of a reaction is when water and iron combine together to form iron oxide
(H2O) (Fe 3) (Fe2 O3)
Another example of a reaction is when zinc and oxygen combine together to form zinc oxide
(Zn) (O2) (Zn O2)
Concentration:
If the concentration is greater so to is the number of particles. When you increase the number of particles you increase the chance of a collision, and the chance of them reacting to form a new product.
Surface area:
The smaller the particles the greater the surface area. Therefore there is a greater chance of them colliding as there is more area for them to hit off. Therefore the smaller the particles the greater the rate of reaction.
Catalyst:
A catalyst is a substance, which speeds up the rate of a reaction, without being used up itself. Catalysts work better when the particles are smaller because the surface area is greater.
Prediction:
I think that the high the concentration the faster the rate of reaction. This is because there is more H+ ions so the higher the chance of colliding. Therefore the quicker the reaction.
Diagram
These are the results I recorded:
Conclusion:
From my results I can conclude that concentration does affect the rate dramatically. For example if we compare strongest strength of acid (1 molar) to the weakest (0.2 molar), there is a difference of nearly 14 seconds between the averages. This is because in the 0.2 molar acid there is only a small amount of h+ ions where as in the 1 molar acid there is a lot more. Therefore the collisions occur a lot faster and the rate of reaction is increased as illustrated in the diagram above.
