• 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
5. 5
5

# Experiment to investigate the stoichiometry of the reaction between copper metal and aqueous silver ions.

Extracts from this document...

Introduction

Copper/Silver Reaction (Stoichiometry) Jason Jie Fong Mr Raj Partners: Kevin Aim To investigate the stoichiometry of the reaction between copper metal and aqueous silver ions. Cu (s) + Ag+ (aq) Cu+2 (aq) + Ag (s) Equipment 250 mL beaker 20 cm copper wire Oven (for drying) Sandpaper Wash bottle 100g 0.1M silver nitrate solution Watch glass 100 mL measuring cylinder ( 1 mL) Safety goggles Rubber gloves Weighing scales Tweezers Safety Precautions: Wear safety goggles at all times. Avoid contact with silver nitrate since it may stain skin and clothing. Method 1) Weigh the 250 mL beaker. 2) Put 100mL of the silver nitrate into the beaker. 3) Wind a 20cm length of Cu wire into an open coil leaving a few cm to act as a handle. 4) Weigh the Cu accurately and then suspend it in the beaker of AgNO3 5) Observe the changes over the next five minutes, then cover the beaker with a watch glass, label the beaker and leave for three days. ...read more.

Middle

Data Processing: Error Calculations: Copper used= Mass of copper before immersion in solution - Mass of copper at the close of the experiment= 0.44g - 0.12g= (0.01/0.44 + 0.01/0.12) � 100 0.32g = +10.6% Mass of Silver (Actual Yield) = Mass of beaker and silver - Mass of Beaker= 117.80g - 116.79g = (0.01/117.80 + 0.01/116.79) � 100 1.01g = +0.0171% For the reaction Cu (s) +2Ag+ (aq) Cu+2 (aq) + 2Ag (s) 0.32g Copper � 63.55g mol-1 = 0.00504 moles (3sf) For every mole of copper there is two moles of silver 0.00504 moles copper � 2 = 0.0101 moles silver (3sf) 0.0101 moles silver � 107.87 g mol-1= 1.08g silver (3sf) Therefore the theoretical yield of silver is 1.09g (3sf). Percentage Yield= (Actual Yield � Theoretical Yield) � 100= (1.01�1.09) � 100= 93.0% (3sf) Therefore the percentage yield is 93.0% (3sf). Conclusion The copper reacted with the silver nitrate to form copper nitrate and a coating on the outside of the copper. ...read more.

Conclusion

This can be avoided by using a measuring cylinder to accurately measure the amount of substance being poured into the beaker. Error Why it's an error Possible improvement Copper could react with other items in its surroundings Copper not involved in the reaction is considered as having participated in the reaction Ensuring the copper is sanded perfectly before being placed inside the beaker, and ensuring the silver nitrate is purely silver nitrate- and water, if the silver nitrate is diluted. Some of the silver nitrate will not have reacted with the copper The silver nitrate that did not react will have been recorded as having reacted. Add the silver nitrate 10mLs at a time and rubbing the silver crystals that form on the copper off every time and collect the crystals, until all of the copper reacted. Then record the amount of silver nitrate added to the copper. The volume of silver nitrate was measured using the marks on the beaker. This systematic error could increase the uncertainty and thus increase the error percentage. Use a measuring cylinder to accurately measure the amount of substance being poured into the beaker. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry 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 International Baccalaureate Chemistry essays

1. ## Testing for halide ions. The objective of the experiment was: ...

* The colour of the three solutions was recorded. * Dilute ammonia(volume= 2*volume of potassium halides) was added in all the solutions, the stoppers were put on all the test tubes, and then the solutions were well shaked to dissolve them. * Concentrated ammonia was added in those solutions which did not dissolve but without stopper on the test tube and then again shaked well.

2. ## Can one determine the coefficients of a balanced chemical equation by having the mass ...

15. Fold the filter paper into eighths and then unfold it in the shape of the filter paper with a little opening near the bottom of the filter paper. This shape ensures that when the paper is put on the funnel, the copper will stay on the paper, while the solution will drip down into the beaker.

1. ## The aim of the experiment is determining the percentage yield of the product (copper), ...

yield is found when the experiment is actually conducted, and it's by weighing the amount of copper, after separating it from the aluminum in the solution. Afterwards, the actual yield is divided by the theoretical, and multiplied by 100, to find out the 'percentage yield'.

2. ## Reactivity series for common metals experiment.

Copper Sulphate(Cu SO4) with: � Copper: No texture/surface/color change (No Reaction) � Iron: A coat of copper appear on the iron and the solution turns pale green. (Reaction) � Magnesium:Turns black on its surface (Reaction) � Zinc: No texture/surface/color change (No Reaction) � Lead: No texture/surface/color change (No Reaction) I.

1. ## Electrolysis of copper sulphate

It is important to repeat experiments when performing any experiment. However, repetition does not improve accuracy of results when systematic errors are present. Systematic errors do not change with repetition and will produce the same inaccurate result with good precision if present.

2. ## Research report on Stoichiometry

These ratios are in moles. ex. O2 + 2 H2 -> 2 H2O The formula shows us that for every ONE O2 atom, there will be a need for TWO H2 atoms to react to make water.

1. ## The balanced equation shows that two moles of silver nitrate react with one mole ...

% uncertainty = ±0.605 Mass of reacted Ag: Uncertainty: m(Ag)= Original weight – final weight m(Ag) = 105.139– 103.335 = 0.001 + 0.001 = 1.804 g = ±0.002 Number of reacted Ag: Uncertainty: Mr(Ag) = 107.87 gmol-1 n(Ag) = 0.0167 mol (3sf)

2. ## Objective: To investigate the order of oxidizing ability of the halogens Cl2, Br2, and ...

Cl2 is more reactive and oxidising agent I2 present and Br2 is oxidizing agent 2. Colour after shaking with KBr solution colourless X Dark red Colour of each layer after shaking with hexane upper colourless X Purple lower colourless X light red Conclusion Br2 present and Cl2 is the stronger oxidizing agent X No visible reaction observed 3.

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