Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the following exothermic reaction: C(s)+2H2(g)⇌CH4(g)?
Coal, which is primarily carbon, can be converted to natural gas, primarily CH4,
by the following exothermic reaction:
C(s)+2H2(g)⇌CH4(g)
A. What is the effect of adding more C to the reaction mixture?
B. What is the effect of adding more H2 to the reaction mixture?
C. What is the effect of raising the temperature of the reaction mixture?
D. What is the effect of lowering the volume of the reaction mixture?
E. What is the effect of adding a catalyst to the reaction mixture?
Would each of these Increase or Decrease Q or K or none of the above.
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C(s) + 2H₂(g) ⇌ CH₄(g)
A.
There is no effect.
This is because the effective concentration of solid is constant even more solid is added.
Both Q and K are unchanged, and Q = K.
B.
The equilibrium position shifts to the right and more CH₄ is formed.
This is because H₂ is removed to counteract the addition of H₂, according to Le Chatelier's principle.
K is unchanged. Before H₂ is added, Q = K. When H₂ is added, Q decreases immediately. Then Q increases and finally Q = K.
C.
The equilibrium position shifts to left and less CH₂ is formed.
This is because the raise in temperature favors the endothermic reaction, i.e. the backward reaction.
Before raising temperature, Q = K. In raising temperature, both Q and K increase. Finally, Q = K.
D.
The equilibrium position shifts to the right and more CH₄ is formed.
This is to lower the number of gaseous molecules to counteract the increase in pressure due to the decrease in volume.
K is unchanged. Originally, Q = K. When volume is lowered, Q decreases immediately. Then Q increases and finally Q = K.
E.
There is no effect because catalyst has no effect on the equilibrium position.
Q = K and both of them are unchanged.