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

The balanced equation shows that two moles of silver nitrate react with one mole of copper

Extracts from this document...


Copper and Silver Reaction Chemistry Internal Assessment Raw data table: What I measured Value (unit) Uncertainty Weight of Beaker 103.335(g) ±0.001g Volume of Silver nitrate 100(cm3) ±1 cm3 Concentration of Silver Nitrate 0.1(mol dm-3) Initial weight of Copper wire 2.020(g) ±0.001g Final weight of copper wire 1.688 ±0.001g Final weight of silver crystals and beaker 105.139 ±0.001g Qualitative Observations: * The copper was a orange/red colour before being submerged. * While the silver nitrate AgNO3 was a clear colourless liquid. * Immediately after the copper was submerged it turned black. * The copper wire was resting on the bottom of the beaker. * After prolonged submersion the wire became thicker as more precipitate was formed on the wire. * After prolonged submersion the solution became a clear light blue solution. * After 24 hours a silver/grey crystalline structure formed around the wire and on the bottom of the beaker. Processed data table: What I measured Value (unit) 3sf Uncertainty Mass of reacted Cu 0.332(g) ...read more.


During the reaction the silver is reduced as it gains electrons and the copper is oxidized as it loses electrons. Cu (s) + 2AgNO3+ (aq) → Cu(NO3)2 (aq) + 2Ag (s) The balanced equation shows that two moles of silver nitrate react with one mole of copper to produce one mole of copper nitrate and two moles of silver. The molar ratio between Copper and Silver should be 1:2, which you can see by the coefficients in the balanced equation. Therefore my hypothesis is wrong as I have 1 more mole of silver than I should have, therefore my mass of silver was larger than expected or the moles of copper was lower than expected and my mass of copper was lower than expected. Yet our small precision error, or random error attributed to the precision of instruments is ±0.716%, which indicates that our range excludes the accepted value of 2. Therefore our must have some experimental error. This experimental error can be determined as a percentage through the following formula: % This experimental error is incredibly large. ...read more.


Another possibility as that during the decanting some crystals were removed from the beaker. This would have decreased the mass of silver, thus decreased the n(Ag) decreasing our ratio. As our ratio was larger than accepted value it is unlikely that this played a significant part in the experimental error of my experiment. To ensure that this would not effect a future experiment I would use a filtration system using filter paper instead of using a decanting method. Experimental error could also have been generated through having an incorrect copper measurement. An incorrect copper measurement could have been caused by copper flecks flaking off the wire into the solution and then being decanted out, though our method did try to remove this possibility by adding more silver nitrate it is still a possibility. This would have meant that we calculated less moles of copper than actually reacted. To ensure that this would not effect our results we should have left the extra silver nitrate for longer to allow it too react with any left over copper flecks. ...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

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Analysis of Silver in an Alloy

    chloride was massed out to � 0.001 on a sensitive balance and dissolved in 25 mL of distilled water. * The precipitate was made by slowly adding the sodium chloride solution to the dissolved silver and stirring with a stirring rod.

  2. Investigate the rate of reaction of luminol in various factors. The objective was to ...

    Concentration (M) y value x value Rate of reaction (y/x) 0.03 0.011 15.161 7.26?10-4 0.06 0.022 17.097 1.29?10-3 0.09 0.215 138.065 1.56?10-3 0.12 0.271 116.774 2.32?10-3 0.15 0.325 101.935 3.19?10-3 0.27 0.035 5.806 6.03?10-3 0.30 0.030 3.87 7.75?10-3 It seems the values are not adequate as some of them are

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

    Record this in "Data Table 1 - Qualitative Data Table" and record it under "Before Reaction". 6. Take 7.50g of copper(ii) chloride salt and spray it with water in a 150mL beaker until the whole salt is dissolved in an aqueous solution.

  2. Effect of Current on The Quantity of Products in Copper Purification Through Electrolysis

    22,4 98 1,575 1,630 1 3 0,5 22,5 98 1,475 1,545 1 4 0,5 23,1 98 1,535 1,590 1 5 0,5 23,5 98 1,535 1,580 1 6 1,5 24,6 98 1,575 1,590 1 7 1,5 24,7 98 1,575 1,615 1 8 1,5 24,9 98 1,525 1,570 1 9 1,5 25,1

  1. Aim: To determine the concentration of chloride ions in sea water by titration ...

    Rinse all apparatus to be used with distilled water. Pat dry using paper towels. 2) Collect sea water in a 100cm3 beaker and mark it as such. 3) Pipette 25cm3 of sea water into the volumetric flask. Tap the pipette lightly against the flask to ensure all of the solution has been transferred.

  2. Relating Moles to Coefficients of a Chemical Equation

    Aim: To find the mole ratio of a reactant to a product in a chemical reaction . Apparatus: - Balance - Bunsen Burner - Two 150 cm3 Beaker - Glass Stirring Rod - Tripod - Gauze - 100 cm3 Graduated Cylinder - Goggles - Heat Proof Mat - Pure Distilled

  1. Electrolysis of copper sulphate

    Sixth current reading is 1.2 amps. Total Quantity of charge = Current Ax TimeS â 1.2 x 120 =144 Coulombs 1. To find number of electrons transferred. Number of e- =Total Quantity of ChargeCharge of 1e- â1441.60217733x10-19= 9 x1020electrons 1.

  2. Research into the production of Nitrate Fertillisers.

    The ammonium fraction is taken up by roots or gradually converted to nitrate by soil microorganisms. Many vegetable growers prefer an immediately available nitrate source of plant nutrition and use ammonium nitrate. It is popular for pasture and hay fertilization since it is less susceptible to volatilization losses than urea-based fertilizers when left on the soil surface.

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