The molar volume of a gas at STP will be experimentally determined using your data from hydrogen gas generation and the combined gas law. However, in our real world, the behavior of cases is not necessarily ideal, and the particles of gases can experience attractions to each other and lose energy in collisions, which is not described in the kinetic molecular theory of gases. At standard temperature (273 K) and pressure (1 atm), the molar volume of a gas 13 -4.7 liters per mole. This volume is referred to as the morar comme of a gas. Based on these principles, at constant conditions of temperature and pressure, 1 more occupies the same volume, regardless of identity. Ideally, all gases exhibit the same behavior, as poverned by the kinetic molecular theory of gases. Additionally, the temperature of your water bath will also serve as the temperature of the hydrogen gas. Based on the temperature of your water bath, you can look up the vapor pressure of you wa page. Therefore, the pressure of your hydrogen gas will be equal to the difference ben pressure in your flask (atmospheric pressure) and the vapor pressure of the water. Dalton's Law states the total pressure of a gas mixture is equal partial pressures of each individual gas in the mixture: Patms = PH2 + PH20 2 The pressure this water vapor exerts contributes to the total re of a gas mixture is equal to the sum of the Florence flask. The vapor pres has a higher vapor pressure because more liquid water increases with temperature warmer water has a higher vapor pressure became rexerts contributes to the total gas pressure in the water evaporates. The pasen water formed above its liquid exerts a pressure called vapor pressure. This evaporation is what happens when puddles disappear after a rainstorm - the water in the puddle turns into a gas. However, water is a liquid that is volatile, which means it can easily evaporate into a gas. The total pressure of gas inside the flask will be made equal to the atmospheric pressure in the laboratory, which will be measured using a barometer, by tilting the base of the flask so as to equalize the level of water inside the flask with the water in the trough. Volume of hydrogen can then be measured by subtracting the amount of water that remains in the flask at the end of the experiment from the total volume of the flask. As the amount of hydrogen increases, the volume of water forced out of the flask will increase. As hydrogen su generated, it will be collected in a flask originally filled with water. The mass of Mg can be The volume of gas generated will be measured via water displacement. The converted to moles of Mg which can then be converted into my V which can then be converted into moles of H, based on the one-to-one ratio given by the balanced equation above. n7 by the reaction shown below and then measure Mg(s) + 2HCl(aq) + MgCl2 (aq) + H2 (9) The mass of magnesium will be measured, while the HCI will be in excess. Thus, a gas are measured, R can be experimentally determine PV R = In this experiment, you will generate hydrogen gas pressure, volume, temperature and moles for the sample. The ideal gas law can be rearranged to when all four quantities that describe a gas are mea must be in moles and the temperature arranged to solve for R as shown below. Note the amount of gas must be in Kelvin. The ideal gas law rela shown in the equation below: Properties - pressure (P) volume (V), temperature crates all of these properties to each other as PV = nRT Where R is the ideal gas constant. Transcribed image text: Experiment 6 Calculating the Molar Vo Wolar Volume of a Gas at STP shown in bount of a measured Gases are described and measured using four prop (T), and amount of gas (n).
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