Equilibrium problem

[yakuza]

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For the following equilibrium, which is endothermic in the forward direction, choose the single correct statement.

CH3CHO (g) --> CH4 (g) + CO (g)

A. A decrease in temperature will increase the pressure in the system
B. Addition of methane will increase the heat absorbed by the system
C. An increase in the volume of the system will increase the total moles of CO at equilibrium
D. at constant total pressure, an increase in temperature will increase the amount of CH3CHO at equilibrium.

The answer is C.

I know for sure B is false and for sure C is true. But can someone explain why A and D are false?

For A, a decrease in temperature will shift the reaction LEFT, which is also the same direction if you increase pressure..so I don't get why its false.

For D, I know CH3CHO would not be increased..............but what does the statement mean by "At constant total pressure"?

 

[osimsDDS]

A is false because as you increase the temperature, b/c its endothermic the temperature is going to be on the left side, so increasing temperature will shift it to the right...then increasing pressure will shift to less moles of gas, which is to the left...so its false

Also temperature and pressure are directly related, increasing temperature increases pressure, here your decreasing temperature and increasing pressure which is not possible

 

[yakuza]

I'm confused on what side heat is on

do I write it as HEAT + CH3CHO (g) --> CH4 (g) + CO (g)?

 

[Danny289]

I'm confused on what side heat is on

do I write it as HEAT + CH3CHO (g) --> CH4 (g) + CO (g)?

yes

 

[avian777]

if it's endothermic, heat will be on reactant side, if exo then it's on product side

 

[avian777]

😡😡

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[rdhdds1]

I'm confused on what side heat is on

do I write it as HEAT + CH3CHO (g) --> CH4 (g) + CO (g)?

Transversly if it is exothermic it (Heat) will be on the right side with the products.