formula: 2Cl- ==> Cl2 + 2e-
in one experiment, the volume of chlorine gas formed was 18cm3.
i) calculate the amount, in moles, of chlorine gas in 18cm3.(the volume of 1 mol of a gas at room temperature and pressure is 24000)
ii) calculate the quantity of electricity, in coulombs, needed to produce this volume of chlorine gas
What's with the same post five times. 24000 what?
24000cm3
I want to get the answer
To calculate the amount of chlorine gas in moles, we need to use the ideal gas law equation, which relates the number of moles of gas to its volume at a specific temperature and pressure. Given that the volume of 1 mole of gas at room temperature and pressure (RTOP) is 24000 cm³, we can use this information to find the number of moles in 18 cm³.
i) Calculate the moles of chlorine gas:
Moles = Volume / Volume of 1 mol
Moles = 18 cm³ / 24000 cm³
Moles = 0.00075 moles
So, the amount of chlorine gas in 18 cm³ is 0.00075 moles.
ii) To calculate the quantity of electricity in coulombs needed to produce this volume of chlorine gas, we need to use Faraday's law of electrolysis, which states that one Faraday of charge is required to produce one mole of an element during electrolysis. One mole of electrons corresponds to 6.022 x 10^23 electrons.
To find the quantity of electricity, we need to convert the number of moles to the number of electrons and then to coulombs.
Quantity of electricity (Coulombs) = Moles x Avogadro's number x Charge of one electron (Coulombs)
Charge of one electron = 1.6 x 10^-19 Coulombs (elementary charge)
Avogadro's number = 6.022 x 10^23 electrons/mole
ii) Calculate the quantity of electricity in coulombs:
Quantity of electricity = 0.00075 moles x (6.022 x 10^23 electrons/mole) x (1.6 x 10^-19 Coulombs/electron)
Quantity of electricity ≈ 7.22 x 10^17 Coulombs
Therefore, the quantity of electricity needed to produce 18 cm³ of chlorine gas is approximately 7.22 x 10^17 Coulombs.