Determine the equilibrium constant for the following reaction at 549 k. ch2o(g) + 2 h2(g) → ch4(g) + h2o(g) δh° = -94.9 kj; δs°= -224.2 j/k determine the equilibrium constant for the following reaction at 549 k. ch2o(g) + 2 h2(g) → ch4(g) + h2o(g) δh° = -94.9 kj; δs°= -224.2 j/k 1.07 x 109 481 2.08 x 10-3 9.35 x 10-10 1.94 x 10-12

The equilibrium constant of the reaction is .

Explanation:

Formula used:

where :

= Gibbs free energy

= Enthalpy of reaction

= Entropy of reaction

R = Gas constant =

T = Temperature in Kelvins

= equilibrium constant at T

So we have:

= ?

= -94.9 kJ/mol = -94900 J/mol

= -224.2 J/mol K

T = 549 K

The equilibrium constant of the reaction is .

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.

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