I have to obtain the water vapor pressure and the partial pressure of butane from two...
I have to obtain the water vapor pressure and the partial pressure of butane from two trials of a Gas Laws experiment. I have my answers, but I am not very confident in my process and answer.
Trial 1: Temperature of Water and Lab: 18.3 c
Mass of Butane released: .028g
Volume of Butane: 16.0g
Barometric Pressure: 626.6 mm Hg
Trial 2: Temperature of Water and Lab: 18.3 c
Mass of Butane released: .013g
Volume of Butane: 15.1g
Barometric Pressure: 626.6 mm Hg
Homework Answers
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I have to obtain the water vapor pressure and the partial
pressure of butane from two...
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water whe...
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water when calculating the moles of hydrogen produced, would the mass of Mg that was calculated at the end of the experiment be too high or too low? nced haf t ribbon are coated with white MgO, would this cause the mass of Mg that you calculate to be too high or too low? Why? 3. Instead of a strip of pure Mg nibbon, you...
DATA Trial 1 Trial 2 Mass of Mg ribbon (g) TO SU 0.07839 (Proom) Barometric pressure...
DATA Trial 1 Trial 2 Mass of Mg ribbon (g) TO SU 0.07839 (Proom) Barometric pressure (mmHg) 756 matte 756rrotta | 22.4°C Temperature of water inside beaker (C) 23.0°C 22.8°C Temperature of the room (°C) (T2) Pwater (mm Hg) Vapor pressure of water found in table at the end of the experiment, based on the temperature of water inside the beaker. 5 mm Hg Volume from graduated cylinder (mL) (V2) 60.2mL 82.4mL CALCULATIONS . Write the balanced chemical equation for...
Please help with these 2 worksheets! I especially am struggling with part D. Trial 1 Trial...
Please help with these 2 worksheets!
I especially am struggling with part D.
Trial 1 Trial 2 Mass of magnesium ribbon 0.04219 Volume of gas collected 0.03869 37 ml 21.0°C Temperature of the gas 43ml 21.1C 29.23inHg Barometric pressure 29.23in its 18.77 torr → 0.71intig 28.509 in Hg Vapor pressure of water 18.65 torr +0.717 into Partial pressure of hydrogen gas 28.513 in Hg Lab Partner: Aya Siblani IV. QUESTIONS and CALCULATIONS A. Calculate the moles of hydrogen gas actually...
A-D A student performed an experiment in which they collected hydrogen gas from the reaction of...
A-D
A student performed an experiment in which they collected hydrogen gas from the reaction of magnesium with hydrochloric acid using the same apparatus that you will be using in today's lab. The reaction is: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) The data they collected are shown below: Mass of Mg Volume of HCI Volume of H2 collected Temperature of H2 collected Barometric pressure 0.100 g 10 mL 57.5 mL 22 °C 29.94 in Hg a. Barometric...
Data Collecting hydrogen gas from the reaction of Mg with HCI Trial 1 Trial 2 Trial 3 Atmospheric pressure (in Hg)...
Data Collecting hydrogen gas from the reaction of Mg with HCI Trial 1 Trial 2 Trial 3 Atmospheric pressure (in Hg) O pen Mass Mg ribbon 0.069 1.osa. 1.069 Volume Ha collected (ml) sim 40 mL de ML Temperature of water (°C) 23 с әət 1 22oC Vapor pressure of water (Table 10.1) 19.8WHO 19.8 mmHg 1.8 in Ho Atmospheric pressure (mm Hg) Partial pressure of H2 Temperature of water (K) Volume of H: collected (L) Moles Hz Theoretical moles...
a student performs this experiment and produces 215 ml of oxygen saturated with water vapor. The...
a student performs this experiment and produces 215 ml of oxygen saturated with water vapor. The temperature is 27 degrees Celsius, atmospheric pressure was 743 mm Hg and the vapor pressure of water at this temperature is 26.7 mmHg. What is the partial pressure of oxygen in this sample? How many moles of oxygen are produced? If the test tube lost 0.258 g of mass during this reaction, what is the molar mass of oxygen?
The Atomic Weight of a Metal Data Trial 2 Trial 1 .036a 37.3mL 22.8°C 33.5ml 22....
The Atomic Weight of a Metal Data Trial 2 Trial 1 .036a 37.3mL 22.8°C 33.5ml 22. 2°C 1. Mass of Magnesium (g) 2. Volume of Hydrogen Gas Collected (mL) 3. Temperature (°C) 4. Temperature (K) (show calculation) 5. Barometric Pressure (mm Hg) Height Difference between Water Levels (mm H,O) tin loin Mercury Equivalent of Height Difference Water Difference (show calculation) 13.6 Vapor Pressure of Water (will be given-mm Hg) Pressure of Dry Hydrogen Gas = Barometric Pressure - Mercury Equivalent...
Im not sure how to calculate the absolute percent error? . Calculate the average molar volume....
Im not sure how to calculate the absolute percent error?
. Calculate the average molar volume. 24.45% mot 23 lunches =47.45 = 23.725 Ymo . Calculate the absolute % error for the average molar volume. Trial 1 Trial 2 Mass of Mg ribbon (g) 10.0541 9 10.07839 Barometric pressure (mmHg) 756 mitte 756mmalta (Proom) Temperature of the room (°C) (T2) Temperature of water inside beaker (°C) 121.060 mmHg 120.615 mm Hg. Pwater (mm Hg) Vapor pressure of water found in...
Lab partner: Molar Mass of Butane Prelab 1. Convert a pressure reading of 875 mm Hg...
Lab partner: Molar Mass of Butane Prelab 1. Convert a pressure reading of 875 mm Hg into atm. (1 atm = 760 mmHg) 2. Look up the chemical formula for butane and calculate its molar mass? 3. A pure gas sample has a volume of 109 mL, a pressure of 723 mm Hg, and a temperature of 23.5°C. Use the ideal gas law (Eq. 1) to calculate how many moles of gas are present in this sample? (Be sure you...
Mass of Magnesium Volume of gas produced Height of water column Trial 2 0.03029 Trial 1...
Mass of Magnesium Volume of gas produced Height of water column Trial 2 0.03029 Trial 1 0.03309 34.4mL 18.26cm 21.7 mmity 23.5°C 751 torr Pressure of water column Temperature of water Atmospheric pressure 23.76 mm Hg 25.0°c 751 torr Water vapor pressure CALCULATIONS: Perform calculations for both trials. 1. Calculate the total pressure of the gases inside the eudiometer at the end of the experiment. Trial 1 Trial 2 2. Calculate the partial pressure of the hydrogen gas in the...
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water when calculating the moles of hydrogen produced, would the mass of Mg that was calculated at the end of the experiment be too high or too low? nced haf t ribbon are coated with white MgO, would this cause the mass of Mg that you calculate to be too high or too low? Why? 3. Instead of a strip of pure Mg nibbon, you...
DATA Trial 1 Trial 2 Mass of Mg ribbon (g) TO SU 0.07839 (Proom) Barometric pressure (mmHg) 756 matte 756rrotta | 22.4°C Temperature of water inside beaker (C) 23.0°C 22.8°C Temperature of the room (°C) (T2) Pwater (mm Hg) Vapor pressure of water found in table at the end of the experiment, based on the temperature of water inside the beaker. 5 mm Hg Volume from graduated cylinder (mL) (V2) 60.2mL 82.4mL CALCULATIONS . Write the balanced chemical equation for...
Please help with these 2 worksheets!
I especially am struggling with part D.
Trial 1 Trial 2 Mass of magnesium ribbon 0.04219 Volume of gas collected 0.03869 37 ml 21.0°C Temperature of the gas 43ml 21.1C 29.23inHg Barometric pressure 29.23in its 18.77 torr → 0.71intig 28.509 in Hg Vapor pressure of water 18.65 torr +0.717 into Partial pressure of hydrogen gas 28.513 in Hg Lab Partner: Aya Siblani IV. QUESTIONS and CALCULATIONS A. Calculate the moles of hydrogen gas actually...
A-D
A student performed an experiment in which they collected hydrogen gas from the reaction of magnesium with hydrochloric acid using the same apparatus that you will be using in today's lab. The reaction is: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) The data they collected are shown below: Mass of Mg Volume of HCI Volume of H2 collected Temperature of H2 collected Barometric pressure 0.100 g 10 mL 57.5 mL 22 °C 29.94 in Hg a. Barometric...
Data Collecting hydrogen gas from the reaction of Mg with HCI Trial 1 Trial 2 Trial 3 Atmospheric pressure (in Hg) O pen Mass Mg ribbon 0.069 1.osa. 1.069 Volume Ha collected (ml) sim 40 mL de ML Temperature of water (°C) 23 с әət 1 22oC Vapor pressure of water (Table 10.1) 19.8WHO 19.8 mmHg 1.8 in Ho Atmospheric pressure (mm Hg) Partial pressure of H2 Temperature of water (K) Volume of H: collected (L) Moles Hz Theoretical moles...
The Atomic Weight of a Metal Data Trial 2 Trial 1 .036a 37.3mL 22.8°C 33.5ml 22. 2°C 1. Mass of Magnesium (g) 2. Volume of Hydrogen Gas Collected (mL) 3. Temperature (°C) 4. Temperature (K) (show calculation) 5. Barometric Pressure (mm Hg) Height Difference between Water Levels (mm H,O) tin loin Mercury Equivalent of Height Difference Water Difference (show calculation) 13.6 Vapor Pressure of Water (will be given-mm Hg) Pressure of Dry Hydrogen Gas = Barometric Pressure - Mercury Equivalent...
Im not sure how to calculate the absolute percent error?
. Calculate the average molar volume. 24.45% mot 23 lunches =47.45 = 23.725 Ymo . Calculate the absolute % error for the average molar volume. Trial 1 Trial 2 Mass of Mg ribbon (g) 10.0541 9 10.07839 Barometric pressure (mmHg) 756 mitte 756mmalta (Proom) Temperature of the room (°C) (T2) Temperature of water inside beaker (°C) 121.060 mmHg 120.615 mm Hg. Pwater (mm Hg) Vapor pressure of water found in...
Lab partner: Molar Mass of Butane Prelab 1. Convert a pressure reading of 875 mm Hg into atm. (1 atm = 760 mmHg) 2. Look up the chemical formula for butane and calculate its molar mass? 3. A pure gas sample has a volume of 109 mL, a pressure of 723 mm Hg, and a temperature of 23.5°C. Use the ideal gas law (Eq. 1) to calculate how many moles of gas are present in this sample? (Be sure you...
Mass of Magnesium Volume of gas produced Height of water column Trial 2 0.03029 Trial 1 0.03309 34.4mL 18.26cm 21.7 mmity 23.5°C 751 torr Pressure of water column Temperature of water Atmospheric pressure 23.76 mm Hg 25.0°c 751 torr Water vapor pressure CALCULATIONS: Perform calculations for both trials. 1. Calculate the total pressure of the gases inside the eudiometer at the end of the experiment. Trial 1 Trial 2 2. Calculate the partial pressure of the hydrogen gas in the...
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