Introduction
An experiment was generated in the lab to enhance the understanding on taking the percent composition and formulating the empirical formula of a hydrate. In chemistry, hydrates are compounds which absorb water molecules and incorporate them as part of a structure. The hydrate in this experiment was an inorganic hydrate, meaning the bonds between water molecules were inadequate (What is a hydrate? (n.d.)). This made it effortless for H2O to detach from the substance when coming in contact with a heating source. This effectively left the substance anhydrous. This experiment determines the number of water molecules related to the hydrate. The experiment also helped formulate the empirical formula and percent composition of the hydrate …show more content…
The substance was stirred until dissolved. The liquid solution produced a blue color as soon as the cupric sulfate dissolved. Prior to this 1.127 grams of Zinc was gathered along with Hydrochloric acid. Both the Zinc and Hydrochloric acid were poured in gradually creating a reaction. A stirring rod was used to stir this while the reaction occurred. Figure 2 shows the reaction in action. Before long less Zinc became visible at the bottom of the beaker. Copper became visible at the bottom of the beaker all at the same time. The bottom of the beaker released bubbles, or hydrogen gas, from the reaction. The reaction for this particular experiment is a single replacement reaction. This means that a single element replaces a second element in a compound. The reaction is shown …show more content…
In the experiment the percent of water and percent of copper can be calculated with the masses that were taken before and after the reaction. The calculations of the percent of water and copper are shown below: Water:
5H2O:(2.194g3.385 g)*100 64.814%
Copper:
Cu:(1.104 g3.385 g)*100 32.614%
When finding the theoretical percent of water and copper one can find the molar mass of each and find the percent. The calculations are shown below:
Water:
5H2O:(90 g153.546 g)*100 58.614%
Copper:
Cu:(63.546 g153.546 g)*100 41.356%
Analysis of results
For this lab the experimental percent is slightly off form the theoretical percent. This is due to error in lab. In step 11, from the lab instructions, a stirring rod was used. This caused loss of Copper in the experiment. Copper was also lost in steps 12 through 15 when decanting the liquid from copper and pouring it into the funnel. Copper particles were left behind in the funnel and could’ve also been decanted. The loss of copper is shown in the calculations since the theoretical percent has a higher percent of copper and the experiment has a lower
An experiment was generated in the lab to enhance the understanding on taking the percent composition and formulating the empirical formula of a hydrate. In chemistry, hydrates are compounds which absorb water molecules and incorporate them as part of a structure. The hydrate in this experiment was an inorganic hydrate, meaning the bonds between water molecules were inadequate (What is a hydrate? (n.d.)). This made it effortless for H2O to detach from the substance when coming in contact with a heating source. This effectively left the substance anhydrous. This experiment determines the number of water molecules related to the hydrate. The experiment also helped formulate the empirical formula and percent composition of the hydrate …show more content…
The substance was stirred until dissolved. The liquid solution produced a blue color as soon as the cupric sulfate dissolved. Prior to this 1.127 grams of Zinc was gathered along with Hydrochloric acid. Both the Zinc and Hydrochloric acid were poured in gradually creating a reaction. A stirring rod was used to stir this while the reaction occurred. Figure 2 shows the reaction in action. Before long less Zinc became visible at the bottom of the beaker. Copper became visible at the bottom of the beaker all at the same time. The bottom of the beaker released bubbles, or hydrogen gas, from the reaction. The reaction for this particular experiment is a single replacement reaction. This means that a single element replaces a second element in a compound. The reaction is shown …show more content…
In the experiment the percent of water and percent of copper can be calculated with the masses that were taken before and after the reaction. The calculations of the percent of water and copper are shown below: Water:
5H2O:(2.194g3.385 g)*100 64.814%
Copper:
Cu:(1.104 g3.385 g)*100 32.614%
When finding the theoretical percent of water and copper one can find the molar mass of each and find the percent. The calculations are shown below:
Water:
5H2O:(90 g153.546 g)*100 58.614%
Copper:
Cu:(63.546 g153.546 g)*100 41.356%
Analysis of results
For this lab the experimental percent is slightly off form the theoretical percent. This is due to error in lab. In step 11, from the lab instructions, a stirring rod was used. This caused loss of Copper in the experiment. Copper was also lost in steps 12 through 15 when decanting the liquid from copper and pouring it into the funnel. Copper particles were left behind in the funnel and could’ve also been decanted. The loss of copper is shown in the calculations since the theoretical percent has a higher percent of copper and the experiment has a lower