find work done when 1mole of calcium carbide reats with water to produce acytelene?
To find the work done when 1 mole of calcium carbide reacts with water to produce acetylene, you need to calculate the change in Gibbs free energy (ΔG) for the reaction. Work done in a chemical reaction is represented by the change in Gibbs free energy, which is a measure of the spontaneity and energy change of the reaction.
The reaction between calcium carbide (CaC2) and water (H2O) to produce acetylene (C2H2) can be written as follows:
CaC2 + 2H2O -> C2H2 + Ca(OH)2
First, you need to find the ΔG° (standard change in Gibbs free energy) for this reaction. You can look up the standard Gibbs free energy of formation values for the compounds involved in the reaction. The ΔG° values can be found in thermodynamic tables or online databases.
Assuming standard conditions (25°C and 1 atm), the ΔG° values for the reactants and products are:
ΔG°f (CaC2) = -59.5 kJ/mol
ΔG°f (H2O) = -237.2 kJ/mol
ΔG°f (C2H2) = 209.2 kJ/mol
ΔG°f (Ca(OH)2) = -942.6 kJ/mol
Next, calculate the ΔG° for the given reaction:
ΔG° = Σ(ΔG°f products) - Σ(ΔG°f reactants)
= [ΔG°f (C2H2) + ΔG°f (Ca(OH)2)] - [ΔG°f (CaC2) + 2ΔG°f (H2O)]
= [209.2 + (-942.6)] - [-59.5 + 2(-237.2)]
= -733.4 kJ/mol
The negative sign indicates that the reaction is spontaneous and releases energy.
Now, the work done (W) can be calculated using the equation:
W = -ΔG
Substituting the value of ΔG into the equation:
W = -(-733.4 kJ/mol)
W = 733.4 kJ/mol
Therefore, the work done when 1 mole of calcium carbide reacts with water to produce acetylene is 733.4 kJ/mol.