K mL K mL K mL c Overall 04215 2 2 T ₁ V ₁ T ₂ V ₂ 2 T ₁ V ₁ T ₂ V ₂ 2 0424

K ml k ml k ml c overall 04215 2 2 t ₁ v ₁

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c. Overall: = = 0.4215 2 + 2 + T V T V 2 + T V T V 2 0.424 +0.419 ° mL ° mL mL 5. % Error = T V T V T V 00% × 1 = 0.398 mL 0.398 − 0.449 mL mL 00% × 1 = -12.8% Boyle’s Law: 1. Constant = P 1 V 1 × a. = (225.06 kPa)(2.8mL) 1. = 630.168 Pa L k · m b. = (191.81 kPa)(4.8mL) 1. = 920.688 Pa L k · m c. = (135.96 kPa)(6.8mL) 1. = 924.528 Pa L k · m d. = (101.75 kPa)(8.8mL) 1. = 895.4 Pa L k · m e. = (83.17 kPa)(10.8mL) 1. = 898.236 Pa L k · m f. = (69.71 kPa)(12.8mL) 1. = 892.288 Pa L k · m Average: = 6 a ) + b ) + c ) + d ) + e ) + f ) = 6 630.168 kPa · mL + 920.688 kPa · mL + 924.528 kPa · mL + 895.4 kPa · mL + 898.236 kPa · mL + 892.288 kPa · mL = 860.218 Pa L k · m = 860 (2 sig figs) Pa L k · m We determined the constant “ ” by multiplying the volume by the pressure for each trial and k then by determining an average from this data. 2. The relationship illustrated by Boyle’s Law is inversely proportional where . As V 1 P the volume increases, the pressure will decrease. Consequently, as the volume decreases, the pressure will increase. V k = P 3. It was necessary to take multiple readings of the dependent variable (pressure) to confirm our observations regarding the relationship from the data in the graph and to minimize percentage of error.
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4. Other gas variables that are required to be kept in certain conditions for Boyle’s Law include temperature and moles. The temperature of the gas needs to be constant throughout the experiment otherwise should the temperature of the gas rise it will cause pressure to increase which will corrupt the data. The temperature of the gas remained constant as it was simply regular air which remained at a constant temperature throughout the duration of the experiment. Moreover, the moles of the gas within the syringe needs to remain constant for the law to work. Should the moles of the gas be increased it will increase pressure as more molecules are hitting the sensor causing the pressure reading to increase. The moles of the gas remained constant as it was just air in the syringe. 5. Discussion: Charles’ Law:
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Based on our data we were able to accurately determine the constant for the equation V 1 T 1 = V 2 T 2 . By doing multiple trials we were able to verify our findings and calculate an average for the constant that we determined. There are several possible sources of error for this experiment. One source of error is that the air could have escaped the erlenmeyer flask during the transportation of the flask from hot water to cold. Another source of error is that a small amount of the water that was left in the flask because of condensation, was not attributed for.
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  • Fall '14
  • Pell, Wendy

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