In this lab, you are producing hydrogen gas in an electrolytic cell. Provide the balanced half reaction for this process? If a student performs this lab and isolates 4 moles of hydrogen, how many moles of
In this lab, you are producing hydrogen gas in an electrolytic cell. Provide the balanced half reaction for this process? If a student performs this lab and isolates 4 moles of hydrogen, how many moles of
In this lab, you are producing hydrogen gas in an electrolytic cell. Provide the balanced half reaction for this process? If a student performs this lab and isolates 4 moles of hydrogen, how many moles of
Calculating Avogadro’s Number Using Electrochemistry Background As discussed in lecture, electrochemistry allows stoichiometric calculations to be related to current and time, if a chemical equation that relates electrons to reactants and products is known. Recall that electrolysis involves using an electrical current to decompose a compound into simpler substances. This particular experiment will involve the electrolysis of a sulfuric acid solution to generate hydrogen gas. By measuring the amount of hydrogen produced by the current and length of time of the electrolysis, it is possible to calculate a value for the Faraday constant and thus also Avogadro’s number. The amount of hydrogen is determined by utilizing the ideal gas law (PV = nRT) to determine the number of moles of hydrogen produced in the electrolysis. The amount of charge that has passed through the solution is measured in coulombs (C). It is calculated by measuring the current (in amperes, A) that has passed through the solution over a known time. Once the charge is known, it is possible, by knowing the amount of hydrogen produced and the stoichiometry of the reaction, to determine Faraday’s constant (the charge in coulombs, C, on one mole of electrons). Furthermore, since the charge of one electron is known (1.60 X 10-19 C) Avogadro’s number can likewise be calculated. Procedure Set up the apparatus as shown on the demonstration table. Place 100 mL of deionized water and 50 mL of 1 M sulfuric acid in a 250 mL beaker. Fill the gas buret completely with this solution and invert it as demonstrated. Making sure that the DC source is unplugged, attach a copper wire to the negative terminal of the DC source and place the other end into the inverted mouth of the gas buret. Be certain that all of the uninsulated wire is inside the buret so that all of the hydrogen is collected. Another copper wire is simply immersed in the solution in the beaker. Read where the top of the solution is in the buret and record this value. Call your instructor to plug in and turn on the DC source, as you begin timing. Record the current (it should start at approximately 0.20 amperes) every thirty seconds so that an average current can be calculated. Do not touch the apparatus while it is plugged in! Continue the electrolysis until at least 10 mL of hydrogen have been collected. Note the time and unplug the DC source. Record the actual volume of hydrogen. Measure the height (in millimeters) of the solution column in the gas buret above the solution in the beaker (i.e. the distance from the top of the solution in the beaker to the top of the solution in the column). Also, measure the temperature of the solution and determine the air pressure in the room.
Lab question 1: In this lab, you are producing hydrogen gas in an electrolytic cell. Provide the balanced half reaction for this process? If a student performs this lab and isolates 4 moles of hydrogen, how many moles of electrons were consumed? If the student calculates that 800000 coulombs of charge were consumed in the production of the 4 moles of hydrogen mentioned above, what is his experimental value for Faraday's constant (the charge on one mole of electrons)?
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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