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The temperature of the gas in Kelvin was 296k. (temperature of water vapor in Celsius) + (273k) = temperature of water vapor in Kelvin The rest of the molar mass of the mixture was fitted by molar mass of hydrogen. 5 units of carbon could fit into the molar mass of the gas mixture. The molar mass of carbon was fitted into molar mass of gas mixture as much as it could without resulting in non-integer number. The mass of the gas mixture was divided by the number of moles of the gas mixture to find the molar mass of the gas mixture.įor finding plausible chemical compound for the molar mass required mix-n-match.
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The difference between the two measurements show the mass of the gas. After the release, the lighter weighted 17.8 g. Before the release, the lighter weighted 17.6 g. To find the mass of the gas mixture, the lighter's mass was weighted for both before and after releasing of the gas. The numbers were plugged in for the PV = nRT equation to find the moles of the gas. The volume of the glass bottle was 262 mL and the volume of water after adding gas mixture was 187 mL. To find the volume of the mixture of the gas, the volume of glass bottle was subtracted by the volume of water left after adding gas to the bottle. Then mmHg was converted to standard atm by dividing the pressured with 760 mmHg. The atmospheric pressure, 760 mmHg, was subtracted by the pressure of the gas, which was 21 mmHg. Using the measured temperature, 23 degrees Celsius, the chart showed that the vapor pressure of water in 23 degrees Celsius was 21 mmHg. To find the pressure, a given chart was used.
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Celsius was converted to Kelvin by adding 273 to 23. It showed that the temperature of the gas was 23 degrees Celsius. To find the temperature, a thermostat was used. The mass of the gas also had to be founded. Because the unit of molar mass is g/mole, finding the number of moles is not sufficient. To find the molar mass of the unknown gaseous compound, the mole of the gas was needed, and to find the mole, PV = nRT equation was used. Using the data and other given information, the molar mass and chemical formula of the gas was calculated. The inside contents of the bottle was locked with the bottle cap and the weight of the bottle filled with water and gas was measured. The bottle trapped the unknown gas and the gas filled the bottle for about one-third. The lighter was also submerged in the water and its gas was released. All of the air bubble was taken out of the bottle. The glass bottle was filled with water and then submerged in the box of water. The weight of the glass bottle, of the lighter, and of the bottle cap was measured. The goal of the lab was to determine the molar mass and the plausible formula of the chemical, using a glass bottle, a lighter, and a handful of laboratory equipments.