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connes 1. Given the following laboratory conditions: barometric pressure = 650 mmHg, temperature of the water...
/2 b) If 1.000 mol of gas occupies 22.711L at STP, and the mass of the...
/2 b) If 1.000 mol of gas occupies 22.711L at STP, and the mass of the vapour in the flask is 530 mg, what is the molar mass of the vapour? C. Further Explorations (Individual Work) 1. Given the following laboratory conditions: barometric pressure 650 mm Hg, temperature of the water bath 97.00 "C and the volume of the Erlenmeyer flask= 145.40 mL a) Determine the volume of the vapour at STP at STP P-760mmH Pa 650mmity T2 Tre Okd273K...
Given: Room temperature: 293.0 K Barometric pressure: 764.0 mmHg Vapor of water: 17.5 mmHg Volume of...
Given: Room temperature: 293.0 K Barometric pressure: 764.0 mmHg Vapor of water: 17.5 mmHg Volume of O2 collected: 68.00 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: A Volume of O2 collected for the unknown: 43.00 mL Calculate the corrected barometric pressure. (mmHg) Calculate the volume of O2 at STP. (mL) Based on the reaction stoichiometry, calculate the number of moles of O2. (moles)...
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...
Date Data Sheet Section Code Table 10.1. Mass, pressure, temperature, and volume measurements. Unknown Number: 924...
Date Data Sheet Section Code Table 10.1. Mass, pressure, temperature, and volume measurements. Unknown Number: 924 Runi Run 2 Run 3 Estimated Error Mass of flask and foil (g) 72.22 72.25 Mass of flask, foil, and condensed vapor (g) 72.39 1241 Temperature of boiling water bath (°C) 100 °C 100°C Volume of Alask (mL) ML 154mL Barometric pressure (mmHg) 754.1754) Room temperature (°C) 22.0021°C Vapor pressure at room temperature (mmHg) 100 °C 100C A student neglected to measure the volume...
1)The barometric pressure is reported to be 695.1 torr and the temperature of the water bath is 22.0 °C. What is the pre...
1)The barometric pressure is reported to be 695.1 torr and the temperature of the water bath is 22.0 °C. What is the pressure (in torr) of dry hydrogen gas in the eudiometer? 2)Calculate the experimental value of the ideal gas constant, R, if 0.00148mol of hydrogen had a volume of 45.5mL at 22.8°C and 0.7771atm. Hint: remember to convert mL to L and °C to K Hint: Answer includes 3 significant figures.
Mass of flask and foil (g) = 63.4842 Mass of flask, foil, and condesned vapor (g) = 63.6995 Temperature of boiling wate...
Mass of flask and foil (g) = 63.4842 Mass of flask, foil, and condesned vapor (g) = 63.6995 Temperature of boiling water bath (C) = 95 degrees C Volume of flask (mL) = 134 Barometric pressre (mmHg) = 763.8 Room temperature (C) = 21.0 degrees C Vapor pressure at room temperature (mmHg) = 100 Find the following: 1) Uncorrected mass of condensed vapor (g) = ? 2). Corrected density of air (g/L) = ? 3). Average volume of flask (L)...
Given a barometric pressure of 747.0 mmHg calculate the pressure of gas sample (a) as indicated...
Given a barometric pressure of 747.0 mmHg calculate the pressure of gas sample (a) as indicated by the manometer (Figure 1) P_gas = Given a barometric pressure of 747.0 mmHg. calculate the pressure of gas sample (b) as indicated by the manometer. (Figure 2) P_gas =
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium...
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium ribbon. 9. Untwist the wire from the piece of fiberglass. Rinse the wire, fiberglass square, and stopper, place them in the container, and return the container to the instructor's desk. The table of temperature/Vapor pressure of water is in your textbook and in the back of your laboratory manual. The density of mercury is 13.6 g/mL. 61302083 Data Sheet Unknown Number Sample 2 40.8m2...
Barometric Pressure 0.992 atm Mass of Flask + Foil 56 g Mass of Flask + Foil...
Barometric Pressure 0.992 atm Mass of Flask + Foil 56 g Mass of Flask + Foil + Condensed Liquid 59 g Mass of Condensed Liquid 3 g Volume of Flask 300 ml Temperature of Water Bath when Vaporization Begins 333 K Temperature of Water Bath when Water Begins to Boil 363 K Molar Mass 46 g mol Ideal gas law PV=nRT P=pressure V=volume of gas n=number of moles R=gas constant T=temperature Molar volume V=RT/P Density of gas D=PM x RT Molar mass M=(mRT)/(PV) I...
Chemistry Charles's Law Post-Laboratory Questions 1. Serveral students performed this experiment without paying adequa...
Chemistry Charles's Law Post-Laboratory Questions 1. Serveral students performed this experiment without paying adequate attention to the details of the procedure. Briefly explain what effect each of the following procedural changes would have ont the size of the volume-to-temperature ratio calculated by the students. A) One student failed to replenish the boiling water in the boiling-water bath as the flask was being heated. At the end of the 6 min of heating, the boiling water in the bath was only...
/2 b) If 1.000 mol of gas occupies 22.711L at STP, and the mass of the vapour in the flask is 530 mg, what is the molar mass of the vapour? C. Further Explorations (Individual Work) 1. Given the following laboratory conditions: barometric pressure 650 mm Hg, temperature of the water bath 97.00 "C and the volume of the Erlenmeyer flask= 145.40 mL a) Determine the volume of the vapour at STP at STP P-760mmH Pa 650mmity T2 Tre Okd273K...
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...
Date Data Sheet Section Code Table 10.1. Mass, pressure, temperature, and volume measurements. Unknown Number: 924 Runi Run 2 Run 3 Estimated Error Mass of flask and foil (g) 72.22 72.25 Mass of flask, foil, and condensed vapor (g) 72.39 1241 Temperature of boiling water bath (°C) 100 °C 100°C Volume of Alask (mL) ML 154mL Barometric pressure (mmHg) 754.1754) Room temperature (°C) 22.0021°C Vapor pressure at room temperature (mmHg) 100 °C 100C A student neglected to measure the volume...
Given a barometric pressure of 747.0 mmHg calculate the pressure of gas sample (a) as indicated by the manometer (Figure 1) P_gas = Given a barometric pressure of 747.0 mmHg. calculate the pressure of gas sample (b) as indicated by the manometer. (Figure 2) P_gas =
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium ribbon. 9. Untwist the wire from the piece of fiberglass. Rinse the wire, fiberglass square, and stopper, place them in the container, and return the container to the instructor's desk. The table of temperature/Vapor pressure of water is in your textbook and in the back of your laboratory manual. The density of mercury is 13.6 g/mL. 61302083 Data Sheet Unknown Number Sample 2 40.8m2...
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