Watch a video of the procedure by clicking here. From the video you will need to record the following data: Volume of H, gas collected in mL: 42.95 mL Height of the water column in cm: 9.3 cm Temperature of water in °C: 23,2 °C Perform the following calculations: 1. Using the balanced chemical equation below, determine the moles of hydrogen gas produced when 0.0408 g Mg reacts. Mg + 2HC1 → MgCl, + H2 2. Convert the height of the water column to the pressure of the water column in mm Hg using the equation below (cm water)x10 13.6 %3D water 3. Determine the pressure of the hydrogen gas if the air pressure was 751.5 mmHg. PH, = P air – P %3D waer 4. Convert the pressure of hydrogen gas from mmHg to atmospheres. mmHg 760 atm = 5. Convert the temperature from Celceus to Kelvin. 6. Determine the volume of hydrogen gas in L 7. Use the ideal gas law, PV = nRT, to determine the value of the R. 8. Based on a value of 0.0821 Latm/molK, determine the percent error for this experiment. experimental value of R-0.0821 0.0821 x 100 Percent Error %D
Watch a video of the procedure by clicking here. From the video you will need to record the following data: Volume of H, gas collected in mL: 42.95 mL Height of the water column in cm: 9.3 cm Temperature of water in °C: 23,2 °C Perform the following calculations: 1. Using the balanced chemical equation below, determine the moles of hydrogen gas produced when 0.0408 g Mg reacts. Mg + 2HC1 → MgCl, + H2 2. Convert the height of the water column to the pressure of the water column in mm Hg using the equation below (cm water)x10 13.6 %3D water 3. Determine the pressure of the hydrogen gas if the air pressure was 751.5 mmHg. PH, = P air – P %3D waer 4. Convert the pressure of hydrogen gas from mmHg to atmospheres. mmHg 760 atm = 5. Convert the temperature from Celceus to Kelvin. 6. Determine the volume of hydrogen gas in L 7. Use the ideal gas law, PV = nRT, to determine the value of the R. 8. Based on a value of 0.0821 Latm/molK, determine the percent error for this experiment. experimental value of R-0.0821 0.0821 x 100 Percent Error %D
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter5: Gases
Section: Chapter Questions
Problem 78QAP
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Question
need help with #8, please show work. Thank you
Transcribed Image Text:Watch a video of the procedure by clicking here. From the video you will need to record the
following data:
Volume of H, gas collected in mL:
42.95 mL
Height of the water column in cm:
9.3 cm
Temperature of water in °C:
23,2°C
Perform the following calculations:
1. Using the balanced chemical equation below, determine the moles of hydrogen gas
produced when 0.0408 g Mg reacts.
Mg + 2HC1 → MgCl, + H,
2. Convert the height of the water column to the pressure of the water column in mm Hg
using the equation below
(cm water)x10
water
13.6
3. Determine the pressure of the hydrogen gas if the air pressure was 751.5 mmHg.
= P
P H2
– P
air
waer
4. Convert the pressure of hydrogen gas from mmHg to atmospheres.
mmHg
atm =
760
5. Convert the temperature from Celceus to Kelvin.
6. Determine the volume of hydrogen gas in L
7. Use the ideal gas law, PV = nRT, to determine the value of the R.
8. Based on a value of 0.0821 Latm/molK, determine the percent error for this experiment.
experimental value of R-0.0821
0.0821
x 100
Percent Error =
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