<p> Gas Laws Lab 1</p><p>Gas Laws Lab</p><p>Name: ______Score: ____/10</p><p>Boyle’s Law:</p><p>Robert Boyle in 1662 first studies the relationship between pressure and volume of a gas at constant temperature. He found that the pressure P of the gas was inversely proportional to its volume V. In other words, if you double the pressure on a given amount of gas, its volume will halve. </p><p>Procedure:</p><p>1. Draw 35 cc (100 cc = 1 L) of air into the syringe and place the cap on the end. </p><p>2. Place the syringe into the wooden blocks. </p><p>3. Place uniform weights (identical books work well) on the top block. After placing each weight, record the volume of air in the syringe and the number of weights added. Tapping the syringe lightly will help reduce errors due to friction. </p><p>Data Table 1: Boyle’s Law Weight Added v. Volume </p><p>Number of Weights Syringe Volume (L) 0 0.035 L </p><p>4. After all the weights have been added and the data recorded, remove them one by one, recording the volume and number of weights as before. </p><p>Data Table 2: Boyle’s Law Weight Removed v. Volume</p><p>Number of Weights Syringe Volume (L) </p><p>1 Gas Laws Lab 2</p><p>0 0.035</p><p>5. Mass each weight that has been added and record the average mass. </p><p>Data Table 3: Mass of Weights</p><p>Number of Weights Mass of Weights (be sure to include units of measurement 1000 g = 1 kg and 2.2 lbs = 1 kg) 0 0.00 kg</p><p>Find the Average Mass (sum of all masses and divide by number of weights)</p><p>6. Disassemble the apparatus and remove the plunger from the syringe. Using a ruler, measure the inside diameter of the syringe barrel. Calculate the area, A, using the formula A = r2 where r is half of the diameter.</p><p>Diameter (cm) </p><p>Radius (m) 100 cm = 1 m</p><p>Area (m2)</p><p>A = r2</p><p>2 Gas Laws Lab 3</p><p>7. Calculate the pressure, P, of each data point by taking the average of the two volumes for each trial, using the relationship: P = F/A, where F is the gravitational force exerted by the weight and A is the area of the syringe barrel. </p><p>Convert Add the Mass (kg) Weight (N) Area (m2) of Pressure = Pressure pressure of Calculate Volume (L ) of weights (m x g) syringe from N/m2 the 1/P g = 10 m/s2 Weight/ Area to atm by atmosphere Average dividing by + 1 atm from tables 1.01 x 10 5 above </p><p>0.00 kg (0.00 x 10) = 4.44 x 10-4 0.00 N/ 4.44 0.00 / 1.01x 0.00+ 1 atm 1/ 1.00 atm 0.035 L 0. 00 m2 x 10-4 m2 = 105 = 0.00 = 1.00 atm = 1 atm-1 Newtons 0 N/m2 atm</p><p>3 Gas Laws Lab 4</p><p>8. Plot the volume, V, versus 1/P for each data point. Record the temperature. </p><p>Temperature: ______(units: ______)</p><p>Graph 1: Volume vs. 1/P for a gas at constant temperature</p><p> Label your axes  Unit of measure on each axis  Scale the axes with even intervals (ex. By 1s, 2s, 5s, etc.)  Plot your data points  Use the best fit line (do NOT connect the dots)  Calculate slope </p><p>Slope = ______Units: ______</p><p>4 Gas Laws Lab 5</p><p>Calculations Page </p><p>5</p>