The oxidation of copper(I) oxide, Cu2O(s) , to copper(II) oxide, CuO(s) , is an exothermic process.
2Cu2O(s)+O2(g)ā¶4CuO(s)
The change in enthalpy upon reaction of 70.64 g Cu2O(s) is ā72.08 kJ .
Calculate the work, š¤ , and energy change, Īšrxn , when 70.64 g Cu2O(s) is oxidized at a constant pressure of 1.00 bar and a constant temperature of 25ā C .
Note that Īšørxn is sometimes used as the symbol for energy change instead of Īšrxn .
To calculate the work, š¤, and energy change, Īšrxn, we need to use the information given and relevant equations.
First, let's calculate the number of moles of Cu2O(s) used in the reaction:
Molar mass of Cu2O = 2 * Atomic mass of Cu + Atomic mass of O = (2 * 63.55 g/mol) + 16.00 g/mol = 143.10 g/mol
Number of moles of Cu2O = Mass of Cu2O / Molar mass of Cu2O
= 70.64 g / 143.10 g/mol
ā 0.493 mol
Now, let's calculate the work using the equation:
š¤ = āPĪš
Since the pressure, P, is given as 1.00 bar and the reaction is taking place at constant pressure, we need to determine the change in volume, Īš.
To find Īš, we use the ideal gas law equation:
PV = nRT
Since the pressure, P, and temperature, T, are given, we need to determine the initial and final volumes, V.
The initial volume, V_initial, can be obtained from the number of moles and molar volume of Cu2O:
V_initial = n_initial * V_molar
The final volume, V_final, can be obtained from the number of moles and molar volume of CuO after the reaction:
V_final = n_final * V_molar
Given that the molar volume at STP (standard temperature and pressure) is 22.4 L/mol, we have:
V_initial = 0.493 mol * 22.4 L/mol
V_final = 4 * 0.493 mol * 22.4 L/mol
Now we can calculate Īš:
Īš = V_final - V_initial
Finally, we can calculate the work:
š¤ = āP * Īš
Next, let's calculate the energy change, Īšrxn, using the equation:
Īšrxn = Īš»rxn - š¤
Given that Īš»rxn is -72.08 kJ, we can substitute the values to find the energy change.
Remember to convert the temperature to Kelvin (25Ā°C + 273.15 = 298.15 K) in order to use the ideal gas law equation.
By following these steps and performing the necessary calculations, you should be able to find the values of work, š¤, and energy change, Īšrxn.