How would each of the folowing changes affect the equilibriumposition for the sy

Question

How would each of the folowing changes affect the equilibriumposition for the system used to produce methanal from carbonmonoxide and hydrogen? CO(g) + 2H2(g) ---CH3OH(g) +heat a. adding CO to the system B.cooling the system C. adding a catalyst to the system D. removing CH3OH from the system E. decreasing the volume of the system How would each of the folowing changes affect the equilibriumposition for the system used to produce methanal from carbonmonoxide and hydrogen? CO(g) + 2H2(g) ---CH3OH(g) +heat a. adding CO to the system B.cooling the system C. adding a catalyst to the system D. removing CH3OH from the system E. decreasing the volume of the system

Explanation / Answer

a. adding CO to the system
Increasing concentration of the reactant ---> equilibrium shiftto product side (to the right)
B.cooling the system
Decreasing temp favors exothermic reactions (reations produce heat)---> equilibrium shift to product side (to theright) C. adding a catalyst to the system
catalyst has no effect on the equilibriumposition
D. removing CH3OH from the system
Decreasing concentration of the product ---> equilibrium shiftto product side (to the right) E. decreasing the volume of the system
decreasing the volume means increasing in pressure. The equilibriumshifts to the side with higher number of gas moles --->equilibrium shift to reactant side (to theleft) (it has 3 moles while the product only has 1mole)

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