Distillation Lab Report
Comparing between the simple and fractional distillation, the fractional distillations for both n-propanol and acetone provided a better distillation. The data and graphs support the statement since the fractional graphs provided a steeper slope than the simple distillation. The steeper slope represent how fast the mixture are separated throughout the distillations. For example, the simple distillation for acetone the slope initially started at about 20 mL at about 65.5℃ and ended at about 30 mL at 101 ℃ in which plateau throughout the distillation. The fractional distillation started to slope at 30 mL at 62℃ and ended at 35 mL at 100℃ as it plateaus until the very end. Similarly, the fractional distillation for n-propanol provided better
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In theory, the temperature difference between water and n-propanol was close at about 2 ℃ difference. In which, while distillation the distilled solution would have both traces of both water and n-propanol. This can be seen in the simple refractive graphs for n-propanol since each consecutive 5 mL have traces of both water and n-propanol. For example, the n-propanol simple refractive graph were spread out throughout the graph with the mole fractions of 0.73, 0.75, 0.83, 0.571. Also, the temperatures are spread out throughout the graphs for both simple and fractional distillation. For example, the simple distillation had its temperature increasing constantly since the initial volume at about 84.2 ℃ until 89.0℃ at 40 mL, in which the temperature skyrocketed at 101.8℃ at 45 mL. Afterwards, the temperature continued to increase steadily until the end of distillation. Similar pattern can been seen with the fractional distillation of n-propanol as initially the temperature increased steadily until at 88.8 ℃ at 35 mL in which skyrocketed to 101.0 ℃ at 40 mL, and remained plateau until the end of distillation. The purity of n-propanol for both simple and fractional came to be 0.0052 mole fraction at 1.3300 refractive index, and 0.0238 mole fraction at 1.3340 respectively. On the other hand, acetone was not azeotropic since the refractive index graphs provided most of the data points were
In theory, the temperature difference between water and n-propanol was close at about 2 ℃ difference. In which, while distillation the distilled solution would have both traces of both water and n-propanol. This can be seen in the simple refractive graphs for n-propanol since each consecutive 5 mL have traces of both water and n-propanol. For example, the n-propanol simple refractive graph were spread out throughout the graph with the mole fractions of 0.73, 0.75, 0.83, 0.571. Also, the temperatures are spread out throughout the graphs for both simple and fractional distillation. For example, the simple distillation had its temperature increasing constantly since the initial volume at about 84.2 ℃ until 89.0℃ at 40 mL, in which the temperature skyrocketed at 101.8℃ at 45 mL. Afterwards, the temperature continued to increase steadily until the end of distillation. Similar pattern can been seen with the fractional distillation of n-propanol as initially the temperature increased steadily until at 88.8 ℃ at 35 mL in which skyrocketed to 101.0 ℃ at 40 mL, and remained plateau until the end of distillation. The purity of n-propanol for both simple and fractional came to be 0.0052 mole fraction at 1.3300 refractive index, and 0.0238 mole fraction at 1.3340 respectively. On the other hand, acetone was not azeotropic since the refractive index graphs provided most of the data points were