• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4

# Investigate the rate of reaction between HCl and Na2S 2O3

Extracts from this document...

Introduction

Planning Investigate the rate of reaction between HCl and Na2S2O3 Jackie Randall 10A For this piece of coursework we are investigating the rates of reaction and he effect different changes have on them. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction. We are studying the affect of changing concentration of Na2S2O3 Solution and dilute HCl. I believe these variables will affect the rate of reaction: * Surface area * Pressure * Temperature * Catalyst * Concentration Concentration If the concentration of a solution is increased there are more reactant particles per unit volume. This increased the probability of reactant particles colliding with each other. Pressure If the pressure is increased the particles in the gas are pushed closer. This increases the concentration and that will change the rate of reaction. Surface Area If a solid is powdered then there is a greater surface area available for a reaction, compared to the same mass of unpowdered solid. ...read more.

Middle

I also predict that as the concentration of the sodium thiosulphate increases the rate of reaction will increase. When the temperature is increased the particles will have more energy and this would enable them to move faster. This will make them collide more often and with more energy. Particles with more energy are more likely to overcome the activation energy barrier to reaction; this would make them react successfully. If solutions of reacting particles are made more concentrated there are more particles in the area. Method Experiment 1 - Changing the concentration 5 cm3 of HCl (at concentration 1 mol./dm3) and 15 cm3 of sodium thiosulphate (at varying concentrations - 10 to 35 g/dm3) are poured out into two measuring cylinders and then poured into a conical flask, which is placed on top of a board marked with letter X. The stopwatch will now be started. When the mixture has turned sufficiently cloudy so that the letter X can no longer be seen the stopwatch will be stopped and the time will be recorded. ...read more.

Conclusion

As the solution gets more concentrated the ions are closer together therefore they will collide more often and more successful collisions are likely, therefore as the concentration decreases fewer successful collisions take place and the rate of reaction slows. Apparatus List * Water Bath * Hazcards * Plastic Pipette * Beaker (250cm3) * Wash bottle * Distilled water * Measuring cylinder (100cm3 and 10cm3) * Flask (250cm3) * HCl (1 Molar) * Stopwatch * Na2S2O3 What I Will Do With My Results... With the results I will use them for creating the following items: * Plot some graphs (Perfect curve, line of best fit) On the axes, I will write: The rate (y axes) and Average time (x axes). * I will also plot the following graph: average times (y axes) and concentration of a) Na2S2O3 b) HCl Strange Results... Potential Variables...Anomalies These are results that are completely out of the blue and therefore most likely to be wrong! I will keep a close eye out for these in my experiments and if I do spot any the experiment will be repeated. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related GCSE Patterns of Behaviour essays

1. ## In my investigation I am going to look at how concentration affects the rate ...

3 star(s)

50 Interpretation and Evaluation My graphs and table agree with my prediction which was that the higher the concentration the quicker the "X" would be obscured by the solution and therefore the higher the rate of reaction. The higher rate of reaction is cause by more particles present in the

2. ## The Rates of Reaction Between HCl and Na2S2O3.

I will only change the one variable, the measurments of HCl and H2O. Also, I will have to pay full attention to the solution when it is reacting so I don't press stop too late. I will have to make sure the solution is kept still because movement will increase the rate of reaction.

1. ## Investigating the effect of temperature on the reaction between Sodium Thiosulphate (Na2S2O3) and Hydrochloric ...

From the straight line I can calculate an equation: y = 0.0008 x - 0.014. From 20�C a rise of 10�C approximately doubled the rate of reaction. From 40�C, however, a rise of 22�C is needed before the rate of reaction is doubled. This shows an increasing rate of reaction.

2. ## Reaction between sodium thiosulphate solution (Na2S2O3) and dilute hydrochloric acid (HCl)

and new bonds are formed (this releases energy). To make this a fair test I will * keep the size of the flask the same (so depth of liquid id is the same) * use the same cross * measure to the same decimal point i.e.

1. ## How much concentration of sodium thiosulphate (Na2S2O3) affects the rate of reaction when tested ...

ions are replaced by the slower-moving bromide ions. Other properties which can be followed in order to determine reaction rates include changes of pressure, for gaseous reactions; changes in optical rotation, where optically active materials are involved; and absorption of electromagnetic radiation, such as light, using a spectrophotometer.

2. ## An investigation into a factor affecting the rate of reaction of sodium thiosulphate (Na2S2O3) ...

I chose rate as opposed to time because I knew that rate was the inverse of time (the reciprocal, or 1/x). This made the curved line straight. Method / Apparatus: conical flask beakers measuring cylinders an "X" card stopwatch sodium thiosulphate hydrochloric acid Firstly I placed the conical flask on top of the "X" card.

1. ## Investigate how temperature affects the rate of reaction of sodium thiosulphate (Na2S2O3) and hydrochloric ...

Thus, when two reactants are mixed, sooner or later a reaction will occur. If the reactants receive more heat energy they will have more kinetic energy - heat and work are closely related.

2. ## ICT modelling spreadsheet - This coursework was designed to investigate the uses of electricity ...

This formula is '=E(row number) x B(row number)'. To do this efficiently, highlight the areas in need to fill, then either click on format...column...fill down, or to do the shortcut, press Ctrl+D. This next formula, is to calculate the individual cost of each item.

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to