For a certain chemical reaction, the standard gibbs free energy of reaction is 144. kj. calculate the temperature at which the equilibrium constant k = 5.9 × 10 . round your answer to the nearest degree.

The question is incomplete, the complete question is:

For a certain chemical reaction, the standard Gibbs free energy of reaction is 144. kJ. Calculate the temperature at which the equilibrium constant K = .

Round your answer to the nearest degree.

25°C is the temperature at which the equilibrium constant is .

Explanation:

where,

= standard Gibbs free energy = 144.0 kJ=144,000 J  (Conversion factor: 1kJ = 1000J)

R = Gas constant =

T = temperature at which reaction is occurring = ?

K = Equilibrium constant of the reaction =

Putting values in above equation, we get:

T = 298.15 K

T = 298.15 - 273 °C = 25°C

25°C is the temperature at which the equilibrium constant is .

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1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%