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Charles's Law, attributed to the pioneering work of J. A. C. Charles and J. L. Gay-Lussac, provides a fundamental insight into the behavior of gases. It posits that, under constant pressure conditions, the volume occupied by a given amount of gas exhibits a direct proportionality to its absolute temperature measured in Kelvin units (Silberberg, 2013). This law serves as a cornerstone in the study of thermodynamics, offering a concise mathematical expression:
The essence of Charles's Law lies in its assertion that as the temperature of a gas increases, its volume expands proportionally, and conversely, as temperature decreases, the volume contracts.
This relationship underscores the intrinsic connection between temperature and volume, shedding light on the dynamic interplay within gaseous systems.
In the context of this experiment, our aim is to delve deeper into the implications of temperature fluctuations on gas volume. Through meticulous observation and analysis, we seek to unravel the intricacies of Charles's Law and discern its practical significance in real-world scenarios.
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By systematically varying the temperature of the gas while holding the pressure constant, we endeavor to elucidate how changes in temperature manifest in alterations to the volume of the gas.
Through this exploration, we endeavor to enhance our comprehension of the underlying principles governing gas behavior. Moreover, we aspire to glean insights that transcend the confines of the laboratory, offering valuable implications for diverse fields ranging from chemistry and physics to engineering and environmental science. Thus, this experiment serves as a gateway to a deeper understanding of the fundamental laws that govern the behavior of matter, paving the way for further inquiry and discovery.
This initial measurement serves as a baseline reference for subsequent calculations and allows us to account for the mass of the apparatus in our analysis.
By meticulously following these procedures, we aim to conduct a systematic and rigorous investigation into the relationship between temperature and gas volume, shedding light on the principles underlying Charles's Law and its practical implications.
Weight of empty equipped flask = 155.05g
Weight of equipped flask and sucked water = 190.52g
Weight of equipped flask and full with water = 354.52g
Weight of water in full flask = 199.47g
Weight of sucked water = 35.47g
Density of water at standard room and temperature = 1g/mL
Volume of sucked water = 35.47mL
Volume of air at 100°C = 199.47mL
Volume of air in room temperature = 164.00mL
Temperature obtained from the graph is -312°C. The theoretical temperature of water is -273°C when the volume of air is 0. The difference between the theoretical and experimental values may be attributed to heat loss from the flask during transportation to the sink.
Using Charles's Law and the volume of gas at 100°C from the experiment, the volume at the water temperature in the sink can be determined:
\( V_2 = \frac{{V_1 \times T_1}}{{T_2}} \)
Substituting the values, \( V_2 = \frac{{199.47mL \times 373K}}{{297K}} = 158.83mL \)
A graph illustrating the theoretical volume of water in the sink was plotted. The graph crosses the temperature axis at -260°C, which deviates from the theoretical value of -273°C. The percent error in the lab was calculated to be 4.76%. Possible errors in the experiment include heat loss from the flask during cooling and inaccuracies in timing.
The temperature of the air in the flask when boiling was recorded as 100°C (T1). Converting this to Kelvin yields 373K. The value of \( \frac{{V_1}}{{T_1}} \) was calculated as 0.53. The volume of air in the flask at the second temperature was measured as 164.00 mL (V2). The temperature of the air in the cooled flask was recorded as 24°C (T2), which converts to 297K. The value of \( \frac{{V_2}}{{T_2}} \) was calculated as 0.55. The close proximity of these values can be attributed to Charles's Law, which states that as temperature increases, so does the volume of a gas sample when pressure is held constant.
The percent error in the lab was 4.76%, indicating potential sources of error such as heat loss and timing inaccuracies. Despite these challenges, the results align closely with theoretical expectations, validating the application of Charles's Law in predicting gas behavior.
In summary, this experiment embarked on a comprehensive exploration of the intricate relationship between temperature and gas volume, as elucidated by Charles's Law. Through meticulous experimentation and detailed analysis, we have uncovered compelling evidence that corroborates the fundamental principles outlined by this law. The alignment between theoretical expectations and empirical findings underscores the robustness and reliability of Charles's Law in describing the behavior of gases under controlled conditions.
However, it is important to acknowledge the presence of minor discrepancies between theoretical predictions and experimental results. While these variations may stem from inherent limitations in experimental procedures or unavoidable sources of error, they provide valuable opportunities for further inquiry and refinement. By critically examining these discrepancies, future research endeavors can uncover new insights and refine existing methodologies, ultimately advancing our understanding of gas behavior and the underlying principles governing it.
Looking ahead, future experiments in this area should prioritize efforts to minimize sources of error and enhance experimental accuracy and reliability. This may involve refining experimental techniques, optimizing equipment design, and implementing stringent quality control measures. Additionally, exploring the influence of external factors, such as pressure and composition, on the relationship between temperature and gas volume could yield valuable insights and broaden the scope of our understanding.
Silberberg, M. S. (2013). Chemistry : The Molecular Nature of Matter and Change (Global Edition). New York: McGraw-Hill.
The Relationship Between Temperature and Gas Volume. (2024, Feb 25). Retrieved from https://studymoose.com/document/the-relationship-between-temperature-and-gas-volume
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