Find the best solutions to your questions at Westonci.ca, the premier Q&A platform with a community of knowledgeable experts. Connect with a community of experts ready to help you find solutions to your questions quickly and accurately. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.

Using standard thermodynamic data at 298k, calculate the free energy change when 2. 34 moles of nh3(g) react at standard conditions

Sagot :

For a thermodynamic data at 298k, when 2. 34 moles of nh3(g) react at standard conditions, the free energy change is mathematically given as

dG'−213.174KJ

What is the free energy change?

Generally, the equation for the Chemical Reaction   is mathematically given as

HCL+NH3----->NH4Cl

Therefore

dG=-202.9-[-16.5+(95.3)]

dG=-91.1KJ/mol

In conclusion, For 2.34 moles

dG'=-91.1KJ/mol*2.34

dG'−213.174KJ

Read more about Chemical Reaction

https://brainly.com/question/1123192

The free energy change when 2.34 moles of NH₃(g) react at standard conditions is -213.174 kJ.

How do we calculate free energy change?

Free energy change of any chemical reaction will be calculated by using the following chemical reaction:

ΔG = Free energy of products - Free energy of reactants

Given chemical reaction is:

NH₃ + HCl → NH₄Cl

From the stoichiometry of the reaction it is clear that same moles of ammonium chloride is produced by the same moles of ammonia & hydrochloric acid.

Free enrgy of NH₄Cl = -202.9 kJ/mol

Free enrgy of NH₃ = -16.5 kJ/mol

Free enrgy of HCl = 95.3 kJ/mol

On putting values in the above equation, we get

ΔG = -202.9-[-16.5+(95.3)]

ΔG = -91.1KJ/mol

For 2.34 moles, ΔG will be:

ΔG = (2.34)(-91.1) = -213.174 kJ

Hence required amount of free eenrgy is -213.174 kJ.

To know more about free energy, visit the below link:

https://brainly.com/question/9063838

#SPJ4