CHM 3/19/19

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Exothermic (∆H<0, heat released)

CO (g) + 3H2 (g) ------> CH4 (g) +H20 (g) ∆H=-206.3 kj (evolved)

^ T <--left

T ---> right

Endothermic (∆H>0, heat absorbed)

CoCl2 (equilibruim arrow) CO + CL2 ∆H=+27.1Kcal

4) Addition of a catalyst does not shift the equilibrium, it just speeds up the time it takes to get to equilibrium

5) Addition of an inert gas at constant volume means there will be no change in the position of the equilibrium

In which direction would the equilibrium be shifted by each of the following applied stresses?

C(s) + H2O (g) equilibrium arrows CO (g) + H2 (g) ∆H = 131 kj

Adding C(s)---->no change

Adding the HE (g) at a constant volume ---->no hcnage

Adding the H2(g) -----> a shift left

Increasing the volume----> shift right

add catalyst ---> no change

increase temp ---> shift right

17-7 The Haber Process-----> Industrial production of NH3 (g)