Calculate Gibbs free energy when S = 131 J mol-1 and H = 155 kJ mol-1 at 25 C, stating whether or not the reaction is feasable.

First, make sure everything is in the correct units: H = 155 kJ mol-1 = 155000 J mol-1 S = 131 J mol-1 T = 25 C = 298K Then use the Gibbs equation to calculate the free energy: G = H - TS G = 155000-298*131 G = 115962 J mol-1 The reaction is not feasible at 25 C as G is positive, therefore temperature must be increased for the reaction to occur

Answered by Isaac H. Chemistry tutor

1687 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How is the electrophile formed for the nitration of benzene??


ii) The maximum permitted sulfate concentration in water is 250mg dm^-3, 200cm^3 of aqueous BaCl2 is added to 300cm^3 of water at the maximum permitted sulfate level, and a white precipitate formed. Calculate the minimum conc. (mol dm^3)of the BaCl2


Calculate the pH change when water is added to 25.0 ml of 0.250M NaOH to form a 1.00l solution.


Describe the changes in equilibrium of ethanol production from ethene and water (enthalpy of reaction is ∆H = - 46 kJ/mol) when: (a) a high pressure is applied; (b) ethanol concentration is increased; (c) temperature is increased; (d) a catalyst is used.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences