• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

How concentration effects the rate of a chemical reaction

Extracts from this document...

Introduction

How concentration effects the rate of a chemical reaction Aim: To show the relationship between the concentration of hydrochloric acid and rate of a chemical reaction. Introduction: I am going to show the relationship between concentration of acid and the rate of reaction. To do this I will measure how long different concentrations of hydrochloric acid take to react then calculate the rate of these reactions. Preliminary work: For my preliminary work I tested which sized calcium carbonate pieces to use, Large, Medium or Powder, and what strength Hydrochloric acid to us, 1M or 2M. ...read more.

Middle

2M hydrochloric acid Safety Goggles Method - Weigh 3g of Calcium Carbonate in each of the 100ml beakers - Connect the conical flask to the gas cylinder via the rubber tube. - Measure 30ml of hydrochloric acid in the 50ml measuring cylinder and put it in to the conical flask - Add 1 beaker (3g) of calcium carbonate to the conical flask, close the bung and start the stop clock. - Every 10 seconds measure the amount of gas in the gas cylinder until either the gas cylinder reaches 100ml+ (full) ...read more.

Conclusion

- Measure 10ml of acid and 20ml of water and repeat. - Measure 5ml of acid and 25ml of water and repeat. - Repeat all 6 experiments at least twice for accurate results. Analysis In conclusion, the more concentrated the acid is, the faster it reacts with the calcium carbonate, therefore meaning that with lower concentration, the rate is lower. If I repeated this investigation I would repeat the experiments more to get a more accurate result, and possibly discount experiments that seem to have different results to the others ...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 Here's what a teacher thought of this essay

This report lacks most of the key elements required in a laboratory report. Suggestions have been made throughout to improve. The basic elements are there but have been omitted from the experimental write up.

Marked by teacher Cornelia Bruce 17/04/2013

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.  Marble Chips and Hydrochloric Acid.

4 star(s)

given off ,which might stay around the magnesium which therefore reduces the surface area of the magnesium and so the acid cannot react properly so this effects the results. 2)We could have controlled factors in the investigation better (e.g the stirring of the solution because if this is�nt done properly it can lead to incorrect results).

2. A-Level Investigation - Rates of Reaction &amp;amp;#150; The Iodine Clock

H2O2, KI and H2SO4. The rate equation can then be written in the form: Rate = k [ H+ ] ? [ H2O2 ]y [ I- ]z ? = Order w.r.t. [ H2SO4 ] y = Order w.r.t. [H2O2 ] z = Order w.r.t.

1. The Iodide - Persulphate Reaction: Determining the Effect of Concentration on Reaction Rate

Run #5 had the extra 15 mL of KNO3 and resulted in a faster reaction rate because it pushes the reaction in the direction that produces more iodine, and this in turn will result in a faster rate of reaction for the same reasons above.

2. Iodine Clock Reaction

9 drops + 1H2O drop 10 drops 6.500 0.1538 0.02349 8 drops + 2H2O drop 10 drops 6.690 0.1495 0.02088 7 drops + 3H2O drop 10 drops 7.400 0.1351 0.01827 6 drops + 4H2O drop 10 drops 9.000 0.1111 0.01566 5 drops + 5H2O drop 10 drops 16.34 0.06120 0.01305

1. Investigation into the effects of trypsin on dried milk solution

and when the concentration had doubled to 0.6% the rate of reaction had also doubled to 0.008364701 (1/sec) this is directly proportional inline with my prediction quickly.

2. To determine the rate law for a chemical reaction among hydrogen peroxide, iodide and ...

used/ cm3 34.55 34.30 Average titre: 34.43cm3 � Trial 1 Reaction Mixture Time/s Temperature/�C A 172 22.0 B 355 22.0 C 91 22.2 D 169 22.1 E 77 32.1 F 56 22.2 Tabble3: Reaction rate measurements Question 1(a) Calculate the order of the reaction with respect to hydrogen peroxide, H2O2.

1. Measuring the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate

measure the loss in mass of the calcium carbonate small chips and record it in the form of graph. This would have been a more accurate result and it would have produced a graph for you.

2. Investigating the rate of reaction between hydrochloric acid and calcium carbonate

CaCo3 (s) + 2HCL(aq) ---> CaCl2(aq) + H20(l) + CO2(g) Salt produced - Calcium carbonate Acid used to neutralize the reaction - Hydrochloric acid This equation tells me the reactants needed and the products produced but doesn't explain how much is needed to for an accurate reaction to take place. • Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to 