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- 1. Determine the value of the ideal gas constant.2. Compare your value of ideal gas constant to the literature value, and calculate the percent error. Mg(s) + 2 HCl(aq) -> H2 (g) + MgCl2(aq) given: Mass of Mg Ribbon: 0.0325g10 mL of 6 M HCl Barometric Pressure: 101.8 kPa Room Temperature: 24.5 oC Water Vapour Pressure: 23.1 mmHg Mass of Mg Ribbon: 0.0325g Initial volume of the Burette: 1.55 mL Final Volume of the Burette: 36.35 mL Height of the Water Column in the Burette: 167.0 mm1) Mass of flask, aluminum foil, and rubber band 68.45g 2) Temp. Of boiling, water 98.20 0C 3) Barometric pressure 755 mmHg 4) Volume of flask (volume of vapor occupies flask) 152 ml 5) Mass of flask, aluminum foil, rubber band, and condensed vapor 68.60g 6) Mass of condensed vapor is (5)-(1) Find Molecular weight of unknown ______ g / mol Calculation PV = (m/M)RT) è M = (mRT) / PV = ? Unknown liquid- Based on Molecular weight determine which unknown below has this molecular weight: Methanol, Ethanol, Isopropanol, Propanol. UNKNOW IS : __________________________The % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. Write the balanced chemical equation of the reaction in your solutions sheet. What is the sum of all the coefficients of the balanced chemical equation? Determine the pressure of the trapped gas inside the eudiometer in mmHg. Determine the partial pressure of the collected CO^2 in mm Hg. How many millimoles of CO^2 was collected? What is the % purity of the sample to the nearest whole number?
- The % purity of a powdered crude sample of Na^2CO^3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What is the % purity of the sample to the nearest whole number?Is it necessary to know [E]T to determine (a) KM, (b) Vmax, or (c) kcat?What is the Molecular weight of a certain volatile liquid which is placed in 225 g flask which has total capacity volume of 251.07 ml where after the liquid was heated to 94.5 oC, the gas volatilized and the weight of the flask measured 227.08g.? Round you answer in one decimal place
- Boyle’s law for confined gases states that if the temperature is constant, pv = c, where p ispressure, v is volume, and c is a constant. At a certain instant the volume is 75 cubic inches, thepressure is 30 psi, and the pressure is decreasing at the rate of 2 psi every minute. What is therate of change of the volume at that instant?A 10.0 mL sample of CO2 is collected by the downward displacement of water at 23.0°C and a room pressure of 100.5 kPa. What is the volume of dry CO2 at 0.00°C and 90.0 kPa?Show complete solutions and enclose all final answers in a box. Round off final answers to 4 decimal places and use floating values for intermediate answers. A gas column is separated into two segments by a non-permeable partition. On the first segment is 1.63 moles of Helium with volume V1 and on the second segment is 3.84 moles of Oxygen gas with volume V2. Consider both gases to be ideal and at the same pressure P and temperature T. If the partition is removed, calculate the change in entropy of the gaseous system.
- Since the specific volume of nitrous oxide gas (N 2 O) at a pressure of 100 kPa and a temperature of 47 ° C multiplied by the compressibility factor is 0.453 m ^ 3 / kg, what is the compressibility factor of this gas?A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g mL-1. The water temperature was 20 ° C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 mL of O2. (11) Calculate the percent error for the experiment. What is the observed molar volume?The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole number