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Identify the correct statement for chang...

Identify the correct statement for change of Gibbs energy for a system `(Delta_(sys)G)` at constant temperature and pressure:

A

if `Delta_(sys)G =0`, the system is still moving in a particular direction.

B

if `Delta_(sys)G lt 0`, the process is not spontaneous

C

if `DeltaG gt 0`, the process is spontaneous

D

if `DeltaG = 0`, the system has attained equilibrium

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To solve the question regarding the change of Gibbs energy for a system (ΔG) at constant temperature and pressure, we will analyze the conditions under which ΔG takes on different values and what those values signify about the spontaneity of a process. ### Step-by-Step Solution: 1. **Understanding Gibbs Free Energy (ΔG)**: - Gibbs free energy (G) is a thermodynamic potential that helps predict the direction of chemical reactions and phase changes at constant temperature and pressure. 2. **Spontaneity of Processes**: ...
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A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) For a system in equilibrium, DeltaG = 0 , under conditions of constant

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) If both DeltaH and Deltas are negative, the reaction will be spontaneous

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