Chemistry lab help

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I need help answers questions for a general chemistry lab. I will provide a couple extra sheets and lab background when I get a bid

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127 An Atoms First Approach to the General Chemistry Laboratory, Second Edition II. Ideal Gas Law Experiment-Experimental Determination of Ideal Gas Constant R 4. Mass of Zn metal: 5. Volume of H2 gas: 6. Atmospheric pressure: 7. Water temperature: 0.237 0.102 g L atm 27.8 °C Analysis 1. Boyle's Law Experiment 8. Volume of air in syringe side of manometer - (length) X 7 X (inner radius)? (#2) XT X [0.5 X (#1)]? cm3 9. Total volume at each step = (volume in syringe) + (volume in long arm of manometer) - (volume in syringe) + (#8) Step (volume in syringe, mL) Total Volume (cm3 or mL) 10. Convert vertical distance between marks (i.e., height difference of water on two sides of manometer) to pressure: Pressure (atm) (height of column of water in mm) (13.5951) X (760) Equation 11 (#3 value) (13.5951) X (760) Gas Laws: Boyle's Law and Experimental Determination of the ideal Gas Constant 153 13-11 Laboratory 13 128 Chem 111 Lab Manual 1/ Pressure Pressure (atm) Step (volume in syringe, mL) 11. Plot [Total volume (L) in #9] vs. [1/pressure (atm) in #10): Laboratory 13 Gas Laws: Boyle's law and An Atoms First Approach to the General Chemistry Laboratory, Second Edition 129 above to a straight line of the form: 12. Using Excel, a graphing calculator, or the least-squares method you utilized in Laboratory 4, fit your data volume - (slope) x ) + (y-intercept) a. Slope of your line (including units): b. Y-intercept of your line (including units): 13. Moles of Zn metal: 14. Moles of H2 produced: 15. Partial pressure of water: II. Ideal Gas Law Experiment-Experimental Determination of Ideal Gas Constant R mol mol atm (use Table 1 below and interpolation) Table 1 Vapor Pressure of Water at Different Temperatures.? Temperature (°C) Water Vapor Pressure (mm Hg) 0 Temperature (°C) Water Vapor Pressure (mm Hg) 5 4.5840 28 28.376 6.5449 10 29 30.071 9.2123 11 30 31.855 9.8483 12 31 33.730 10.522 13 32 35.700 11.237 14 33 37.769 11.993 15 34 39.942 12.795 16 35 42.221 13.642 36 17 44.613 14.539 37 18 47.121 15.487 38 19 49.750 16.489 39 52.506 20 17.546 40 55.391 21 18.663 45 71.968 22 19.841 50 92.648 23 21.085 60 149.61 24 22.395 70 234.03 25 23.776 80 355.63 26 25.231 90 526.41 27 26.763 100 760.00 13-13 Laboratory 13 Gas Laws: Boyle's Law and Experimental Determination of the ideal Gas Constant 155 130 atm 16. Pressure of H, gas - PH20 (#6) - (#15) mol (#16) - (#5) (#13) X (#7 in K Р P XV а n XT 17. Experimental R = 18. % error (experimental R vs. literature value for R): Reflection Questions 1. (a) In your plot of V vs. 1/P, what is the numerical value for the slope? (b) Based on the ideal gas law, what does the slope of this best-fit line represent? (c) What do you expect the y-intercept of the best-fit line to equal? (d) If you assume the temperature in the room was 20.0°C when you conducted the Boyle's law experiment, how many total moles of gas were in the trapped volume (i.e., within the syringe plus within the tubing between the water and the syringe)? 2. Using ideas from the kinetic molecular theory, explain why pressure increases as volume decreases, Laboratory 13 Gas Laws: Boyle's Law and Experimental Determination of the ideal Gas Constant
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Explanation & Answer

here is the graph

Volme vs 1/P
500
400

pressure/atm

Total volume(L) 1/P (a...


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