Relating Moles to Coefficients of a Chemical Equation Essay

Introduction The definition of a mole is Avogadros number (6.02 x 1023) of particles (atoms, molecules, ions, electrons etc.). Moles ar a very important part of chemistry especially in stoichiometry since it is part of many other calculation quantities and formulas including molar mass, solution calculations and gas intensity calculations.The mole is also used in chemical reactions and equations to calculate the derive of reactant needed to react completely with another reactant or to calculate the product produced from the amount of reactant provided and vice versa. This is done by using the proportion of the coefficients in a balanced equation. This ratio of coefficients is also known as the mole ratio.In the sideline experiment, a simple displacement reaction would occur from the reaction of an aqueous solution of slob (II) sulphate and surface powder.Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s)This reaction would be set up to allow the zinc to be the limiting factor therefore react completely, in order for that to happen, papal bull (II) sulphate would be in excess. As zinc is the limiting factor, it will be used to calculate the expected amount of copper produced from the 1 to 1 mole ratio of zinc and copper from the balanced equation above.Aim To find the mole ratio of a reactant to a product in a chemical reaction . tool Balance Bunsen Burner Two cl cm3 Beaker Glass Stirring Rod Tripod Gauze 100 cm3 Graduated Cylinder Goggles Heat Proof phlegm Pure Distilled Water Tongs Balance to 0.01 gReagents Copper (II) Sulphate Crystals Zinc PowderMethod1. Weigh the mass of a clean, dry 150 cm3 beaker. Then weigh out 7.0 g of copper (II) sulphate using the beaker2. Add 50.0 cm3 of virgin distilled water into the beaker and heat the solution gently until all the copper (II) sulphate has dissolved3. Determine the mass of the second clean, dry 150 cm3 beaker. Then weigh out as accurately as possible, 1.30 g of zinc powder using the beaker4. Record the mas s of the beaker and the zinc powder in the results table, nearest to 0.01 g5. Slowly pour the copper (II) sulphate into the beaker containing the zinc. Stir always for 1-2 minutes6. Leave the beaker for 10 minutes while the reaction continues. Record your observations7. When the copper has settled, pour out the light blue liquid.8. Add 10 cm3 of pure distilled water into the beaker.9. Leave it for 10 minutes again and pour out the liquid again10. Repeat steps 8 and 9, two times11. line the beaker in the oven to dry for 24 hours12. Remove the beaker from the oven and determine the mass.Results1. Mass of desolate 250 cm3 beaker97.37g2. Mass of the 250 cm3 beaker and copper (II) sulphate104.37g3. Mass of copper (II) sulphate7.0g4. Mass of empty 150 cm3 beaker98.66g5. Mass of 150 cm3 beaker and zinc powder99.96g6. Mass of zinc powder1.30g7. Mass of the 150 cm3 beaker and copper formed (after drying overnight)98.78g8. Mass of copper1.41gCalculations1. routine of moles of copper produ cedn === 0.0222 mol2. Number of zinc moles reactedn === 0.0199 mol3.ZnCu0.0199 mol0.0222 mol114. Mass of copper expected=n(Cu) = 1 x 0.0199= 0.0199 molm = nM= 0.0199 x 63.55= 1.26 g5. Percentage Yieldx 100= 89.4%Conclusion The mole ratio from calculation 3 is approximately 1 to 1, same as the expected mole ratio from the balanced equation. The expected mass of copper is 1.26 g however 1.41g of copper was weighed out therefore, the persona yield of the above experiment is 89.4%. This is mostly caused by the impurity of the copper since there might be a delicate amount of leftover zinc sulphate in the beaker.Evaluation From the experiment above, some things could have been done better to achieve a higher percentage yield. The trumpery rod shouldve been dipped into water before stirring the copper (II) sulphate and zinc in order for no copper to attach to the glass rod after stirring. More importantly, I could have improved and made this experiment more accurate by rinsing the copp er more thoroughly so no zinc sulphate would be left in the beaker.