Title: Stoichiometry to Calculate Reaction of Zinc and Iodine and Law of Conservation of Mass
Authors: Sang Nguyen and Sami Biro
Introduction
II. Materials and Methods
A. Materials
Zinc (Zn), iodine (I2), acetone (C3H6O), acetic acid (C2H4O2) and zinc iodide (ZnI2) were used to conduct this experiment in order to confirm the validity of the law of conservation of mass as well as to use Stoichiometry to calculate the reaction between zinc and iodine.
There are some precautions that one must consider before handling and using these specific chemicals. All of the chemicals used impose at the minimal, hazard to skin and eyes. However, acetic acid in particular can be very hazardous with skin, eyes and inhalation and can potentially damage tissues according to the MSDS.
B. Method 1
To set up the reaction between zinc and iodine (known as trial 1), 2.0 grams of zinc was first obtained and placed into a labeled test tube 1. After, 2.0 grams of iodine was used as well in the tube. Then, 5mL of dilute …show more content…
Result 1
1. In trial 1, the mass of zinc iodide was 2.51 grams.
2. Although, the consumed moles and mass of zinc consumed could not be calculated due to an accident during lab, the mass of iodine consumed was 2.0 grams and moles consumed was 0.0079 moles. The theoretical yield for the zinc iodide was 2.51 grams and 2.51 grams was produced which makes the actual or experimental yield 100%.
3. The possible errors could have occurred due to human error in calculations or mis-calculations in the weighing process of mass of the 250mL beaker. For example, the tape on the beaker could make the mass slightly higher than it actually should be.
B. Result 2
1.In trial 2, 0.05 grams of zinc was consumed and 7.70 x 10^-4 moles of zinc consumed. While total mass of iodine consumed was 1.7 grams and 0.00669 moles of iodine was consumed. In trial 3, 0.54 grams of zinc was consumed and 0.00830 moles was consumed. In addition, 1.4 grams of iodine was consumed and 0.0051 moles was
Authors: Sang Nguyen and Sami Biro
Introduction
II. Materials and Methods
A. Materials
Zinc (Zn), iodine (I2), acetone (C3H6O), acetic acid (C2H4O2) and zinc iodide (ZnI2) were used to conduct this experiment in order to confirm the validity of the law of conservation of mass as well as to use Stoichiometry to calculate the reaction between zinc and iodine.
There are some precautions that one must consider before handling and using these specific chemicals. All of the chemicals used impose at the minimal, hazard to skin and eyes. However, acetic acid in particular can be very hazardous with skin, eyes and inhalation and can potentially damage tissues according to the MSDS.
B. Method 1
To set up the reaction between zinc and iodine (known as trial 1), 2.0 grams of zinc was first obtained and placed into a labeled test tube 1. After, 2.0 grams of iodine was used as well in the tube. Then, 5mL of dilute …show more content…
Result 1
1. In trial 1, the mass of zinc iodide was 2.51 grams.
2. Although, the consumed moles and mass of zinc consumed could not be calculated due to an accident during lab, the mass of iodine consumed was 2.0 grams and moles consumed was 0.0079 moles. The theoretical yield for the zinc iodide was 2.51 grams and 2.51 grams was produced which makes the actual or experimental yield 100%.
3. The possible errors could have occurred due to human error in calculations or mis-calculations in the weighing process of mass of the 250mL beaker. For example, the tape on the beaker could make the mass slightly higher than it actually should be.
B. Result 2
1.In trial 2, 0.05 grams of zinc was consumed and 7.70 x 10^-4 moles of zinc consumed. While total mass of iodine consumed was 1.7 grams and 0.00669 moles of iodine was consumed. In trial 3, 0.54 grams of zinc was consumed and 0.00830 moles was consumed. In addition, 1.4 grams of iodine was consumed and 0.0051 moles was