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What is the value for (delta)G at 1000 K if (delta)H = -220 kJ/mol and (delta)S = -0.05 kJ/(molK)?

A. -220 kJ
B. -270 kJ
C. 780 kJ
D. -170 kJ

Respuesta :

Hagrid
The system is isothermal, so we use the formula:
(delta)G = (delta)H - T (delta) S

Plugging in the given values:
(delta)G = -220 kJ/ mol - (1000K) (-0.05 kJ/mol K)
(delta)G = -170 kJ/mol

If we take a basis of 1 mol, the answer is
D. -170 kJ 

The value of ΔG is -170 kJ/mol at 1000 K if ΔH is -220 kJ/mol and ΔS is -0.05 kJ/mol K.

Hence, option (D) is correct answer.

What is Gibbs Free energy ?

Gibbs free energy is also called free energy, free enthalpy, Gibbs energy which is used to measure the capacity of a system to do work in a  thermodynamic system. It is denoted by the symbol 'G'.

How to calculate the Change in free energy (ΔG) ?

To calculate the change in free energy as

ΔG = ΔH - T ΔS

where,

ΔG = Change in free energy

ΔH = Enthalpy change

T = Temperature in Kelvin

ΔS = Entropy change

Now put the value in above formula we get

ΔG = ΔH - T ΔS

     = -220 kJ/mol - (1000 K) (-0.05 kJ/mol K)

     = -220 + 50

     = -170 kJ/mol

Thus, from above conclusion we can say that The value of ΔG is -170 kJ/mol at 1000 K if ΔH is -220 kJ/mol and ΔS is -0.05 kJ/mol K.

Hence, option (D) is correct answer.

Learn more about the Gibbs Free energy here: https://brainly.com/question/13765848

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