Calculate the standard free energy change at 25°c the following reaction 3Cu+2NO3+8H->3Cu+2NO+4H2O
358924.2J
Calculate the standard Free energy change at 25 degrees Celsius for the following reaction 3Cu+2No3+8H-3Cu2+2No+4H2
I rewrote the equation to make it more acceptable.
3Cu + 2[NO3]^- + 8H^+ -> 3Cu^2+ + 2NO + 4H2O
Look up the standard free energy of EACH of the products and reactants from a table in your text/notes/web and apply as follows:
dGo reaction = (n*dGo products) - (n*dGorreactants)
Post your work if you get stuck.
To calculate the standard free energy change (ΔG°) for a reaction at 25°C, you can use the equation:
ΔG° = ΔH° - TΔS°
where:
- ΔG° represents the standard free energy change,
- ΔH° is the standard enthalpy change,
- T is the temperature in Kelvin, and
- ΔS° is the standard entropy change.
To proceed, we need the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°) for the reaction.
Firstly, we'll need to balance the given reaction equation properly:
3Cu + 2NO3 + 8H -> 3Cu + 2NO + 4H2O
It seems that some of the reactant and product species are missing charges or states (e.g., Cu+, NO3-, NO). For a more accurate calculation, we need the correctly balanced and indicated charges and states of every species involved.
Once you've provided the balanced equation and necessary details, we can proceed with calculating the standard free energy change.