The ? H ? for the reaction above is +252 kJ. The system is initially at equilibr

Question

The ?H? for the reaction above is +252 kJ. The system is initially at equilibrium. What happens if CH4 is added to the reaction mixture at constant temperature and volume? (Select all that apply.)

The reaction absorbs energy.

The reaction releases energy.

[CH4] increases.

[CH4] decreases.

[CH4] remains consant.

[O2] increases.[O2] decreases.

[O2] remains constant.

CH3OH] increases.

[CH3OH] decreases.

[CH3OH] remains constant.

The ?H degree for the reaction above is +252 kJ. The system is initially at equilibrium. What happens if CH4 is added to the reaction mixture at constant temperature and volume? (Select all that apply.) The reaction absorbs energy. The reaction releases energy. [CH4] increases. [CH4] decreases. [CH4] remains consant. [O2] increases.[O2] decreases. [O2] remains constant. CH3OH] increases. [CH3OH] decreases. [CH3OH] remains constant.

Explanation / Answer

Uhh i'll help with the first one and give you the idea of how to do it. If delta H is positive, the reaction is endothermic, meaning it absorbs energy. Based on le Chatelier's principlehttp://en.wikipedia.org/wiki/Le_Chatelie... If you add something to an equilibrium, it shifts in the opposite direction. So if you add CH4, then CH3OH increases and CH4 and O2 decrease.

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