Homework Answers
Trial 1
Molar mass of Mg = 24.3 g/mol
Moles = mass /molar mass = 0.044 /24.3 = 0.0018 moles
Trial 2
Mass of Mg reacted = 0.04 gram
So moles of Mg reacted = 0.04/24.3 = 0.00164 moles
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moles of Mg reacted for Trial 1 and Trial 2. show calculations Trial Trial 1 Measured...
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...
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...
i need help with the moles of H2 gas please Trial 1 Trial 2 Mass of...
i need help with the moles of H2 gas please
Trial 1 Trial 2 Mass of Mg ribbon (e) 10.0541 g 0.07839 Barometric pressure (mmHg) (Proom) 1 75 66 matts 756 mutta Temperature of the room (°C) 224 °C 22.4 °C Temperature of water inside beaker (°C) 23.0°C 22.8°C (T2) Pwater (mm Hg) Vapor pressure of water found in table 21.068 van Hg 20.615 mm Hg at the end of the experiment, based on the temperature of water inside the...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
moles of Mg and balanced chenical reactions with phases Name: Haytry Stonavina Data Section #: Date:...
moles of Mg and balanced chenical reactions with phases
Name: Haytry Stonavina Data Section #: Date: Collecting hydrogen gas from the reaction of Mg with HCI TO HG Atmospheric pressure in Hg) Mass Mg ribbon Volume Ha collected (ml) Temperature of water (°C) 11 Partial pressure of H: Temperature of water (K) Trial 1 Trial 2 Trial 3 1 7600 nano 700 ruilo osolog .059 1.089 sime 46 ML I de ML 22°C 22°C 12°c 19.8 mmHg 19.8 amHg 19.8...
9->moles Data Table - Mg with HCI nga2 + H₂ Ptoral - Plzo =PHz Trial 1...
9->moles Data Table - Mg with HCI nga2 + H₂ Ptoral - Plzo =PHz Trial 1 Trial 2 Mass of magnesium Atmospheric pressure 0319 767.4 mmHg 17.5mm Hg -0429 767.4 mmHg 17.5mmites Partial pressure of water (Table 11.1) Pressure of dry hydrogen gas Volume of hydrogen gas 30-70 mL 201°C 43.05ml 20.1°C Temperature of hydrogen gas Calculate the number of moles of dry hydrogen gas for each trial from mass of Mg metal Calculate the gas constant, R, for each...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Data provided solve Q3 and Q4 please Table 2. Experimental Data Trial 1 Trial 2 Trial...
Data provided
solve Q3 and Q4 please
Table 2. Experimental Data Trial 1 Trial 2 Trial 3 30.13 Atmospheric Pressure (inches Hg) Mass Mg used (8) 0.039 0.025 0.011 39.58 25.89 11.47 Volume Hz gas generated (mL) Water Temperature (°C) 19.0 19.0 19.0 16.48 16.48 16.48 Partial Pressure Water Vapor (mm Hg; from Table 1) Difference in Water Levels (mm) 14.31cm 35.72cm 46.13cm Table 3. Molar Gas Volume and Ideal Gas Constant Calculations Trial 1 Trial 3 Trial 2 Trial...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of wat...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
Section - Date Name Lab Partner DATA Trial Mass of Mg (g) - 0.0301 3 Temperature...
Section - Date Name Lab Partner DATA Trial Mass of Mg (g) - 0.0301 3 Temperature (°C) Volume of H, gas (mL) 30.1 Barometric Pressure (mmHg)_latm 349 38.6 lamm CALCULATIONS A. Experimental Determination of the gas constant, R 1. Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid 2. How many moles of Mg were consumed? 3. Based upon the chemical equation how many moles of H, gas were produced? 4. What volume of H, gas...
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...
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...
i need help with the moles of H2 gas please
Trial 1 Trial 2 Mass of Mg ribbon (e) 10.0541 g 0.07839 Barometric pressure (mmHg) (Proom) 1 75 66 matts 756 mutta Temperature of the room (°C) 224 °C 22.4 °C Temperature of water inside beaker (°C) 23.0°C 22.8°C (T2) Pwater (mm Hg) Vapor pressure of water found in table 21.068 van Hg 20.615 mm Hg at the end of the experiment, based on the temperature of water inside the...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
moles of Mg and balanced chenical reactions with phases
Name: Haytry Stonavina Data Section #: Date: Collecting hydrogen gas from the reaction of Mg with HCI TO HG Atmospheric pressure in Hg) Mass Mg ribbon Volume Ha collected (ml) Temperature of water (°C) 11 Partial pressure of H: Temperature of water (K) Trial 1 Trial 2 Trial 3 1 7600 nano 700 ruilo osolog .059 1.089 sime 46 ML I de ML 22°C 22°C 12°c 19.8 mmHg 19.8 amHg 19.8...
9->moles Data Table - Mg with HCI nga2 + H₂ Ptoral - Plzo =PHz Trial 1 Trial 2 Mass of magnesium Atmospheric pressure 0319 767.4 mmHg 17.5mm Hg -0429 767.4 mmHg 17.5mmites Partial pressure of water (Table 11.1) Pressure of dry hydrogen gas Volume of hydrogen gas 30-70 mL 201°C 43.05ml 20.1°C Temperature of hydrogen gas Calculate the number of moles of dry hydrogen gas for each trial from mass of Mg metal Calculate the gas constant, R, for each...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Data provided
solve Q3 and Q4 please
Table 2. Experimental Data Trial 1 Trial 2 Trial 3 30.13 Atmospheric Pressure (inches Hg) Mass Mg used (8) 0.039 0.025 0.011 39.58 25.89 11.47 Volume Hz gas generated (mL) Water Temperature (°C) 19.0 19.0 19.0 16.48 16.48 16.48 Partial Pressure Water Vapor (mm Hg; from Table 1) Difference in Water Levels (mm) 14.31cm 35.72cm 46.13cm Table 3. Molar Gas Volume and Ideal Gas Constant Calculations Trial 1 Trial 3 Trial 2 Trial...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
Section - Date Name Lab Partner DATA Trial Mass of Mg (g) - 0.0301 3 Temperature (°C) Volume of H, gas (mL) 30.1 Barometric Pressure (mmHg)_latm 349 38.6 lamm CALCULATIONS A. Experimental Determination of the gas constant, R 1. Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid 2. How many moles of Mg were consumed? 3. Based upon the chemical equation how many moles of H, gas were produced? 4. What volume of H, gas...
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