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K brings a process including delta g into equilibrium in a reaction. The two work together to maintain a reaction's equilibrium keeping it stable and helping it to continue at a stable rate.

Q: How is delta g related to K?

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Some words containing k, g, w:knowingtweakingwakingwalkingwhackingwinking

K as in asdfghjk across you keyboard

gok (name)

backgammongimmickkingdomkingmakermakingmarketingmarkingmilkingmistakingmockingremarkingsmackingsmockingsmoking

G is the midway letter between C and K.

Related questions

If ΔG is negative, it means the reaction is spontaneous in the forward direction. In this case, the equilibrium constant K will be greater than 1, indicating that the reaction favors the products at equilibrium.

To calculate the value of ΔG at 500 K, you can use the equation ΔG = ΔH - TΔS. Given ΔH = 27 kJ/mol, ΔS = 0.09 kJ/(mol K), and T = 500 K, plug in the values to find ΔG. ΔG = 27 kJ/mol - (500 K)(0.09 kJ/(mol K)) = 27 kJ/mol - 45 kJ/mol = -18 kJ/mol. Therefore, the value of ΔG at 500 K is -18 kJ/mol.

Delta G (written triangle G) = Delta H -T Delta S

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Delta G (written triangle G) = Delta H -T Delta S

G is always positive when enthalpy increases and entropy decreases.

Photosynthesis is a positive delta G as it produces more free energy than it uses. The overall result of the Gibbs equations shows that delta G is positive

The specific heat can be calculated using the formula: ( q = mc\Delta T ), where ( q ) is the heat absorbed, ( m ) is the mass, ( c ) is the specific heat, and ( \Delta T ) is the temperature change. Plugging in the values: ( 67.2 = (44.0) \times c \times 11 ), solving for ( c ) gives a specific heat of approximately 0.138 J/g∙K.

The change in enthalpy between products and reactants in a reaction

Delta S represents the change in entropy of a system. In the equation delta G = delta H - T delta S, it is used to determine the contribution of entropy to the overall change in Gibbs free energy. A negative delta S value suggests a decrease in the disorder of a system.

Doubling the amount of enzyme does not affect delta G, as delta G is a thermodynamic property that depends on the free energy difference between the products and reactants in a reaction. Enzymes lower the activation energy of a reaction but do not change the overall free energy change.

The change in enthalpy between products and reactants in a reaction