What is deltaG at 298 K for the reaction
C + O2 = CO

The answer for the following problem is mentioned below.

Therefore the Gibbs free energy (ΔG) for the reaction is -394.36 J

Explanation:

Given:

ΔH = -393.5 kJ/ mol

ΔS =0.0029 kJ/mol K

T = 298 K

To solve:

Gibbs free energy (ΔG)

We know;

ΔG = ΔH - TΔS

ΔG  = -393.5 - (298 × 0.0029)

ΔG = -393.5 - 0.8642

ΔG = -394.36 J

Therefore the Gibbs free energy (ΔG) for the reaction is -394.36 J

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

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