chemistry

posted by .

the reaction CO + 2H2<----->CH3OH has a delta H -18 kJ. how will the amount of CH3OH be affected by the following.

a) removing H2(g)
b) decreasing the volume of the container.

  • chemistry -

    This is a question on Le Chatelier's Principle. Basically that principle tells us that a system in equilibrium will try to undo what we do to it. That isn't what you read in a text but it is one way to look at it.
    So if we ADD H2 to the system it will try to undo that. How can it do that? By using up the added H2 of course. So the reaction will shift to the right (producing more CH3OH at the expense of H2 and CO). Increasing pressure will shift it to the side with FEWER moles. Take this information and answer the questions.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    1.2 mol of CH3OH(g) are injected into a 2.0 L container and the following equilibrium becomes established. 2H2(g) + CO(g) <=====> CH3OH(g) + 92 kJ If at equilibrium 1.0 mol of CH3OH is still in the container the Ke must be which …
  2. Chemistry

    How many CO2 molecules would be formed from the reaction mixture that produces the greatest amount of products?
  3. chemistry

    2. Methanol, CH3OH, is used as fuel in race cars. This liquid fuel can be synthesized using the following process C(s)+ ½ O2(g) + 2H2(g)  CH3OH(l) Calculate delta G using the deta Gf of the reaction. Calculate Kp. What is …
  4. College Chemistry

    Consider the evaporation of methanol at 25.0 C: CH3OH(l)--->CH3OH(g) Delta G= 4.3 kJ Find Delta G at 25.0 C under the following nonstandard conditions: Pressure of CH3OH= 108.0 mmHg.
  5. Chemistry

    Consider the evaporation of methanol at 25.0 C: CH3OH(l)--->CH3OH(g) Delta G= 4.3 kJ Find Delta G at 25.0 C under the following nonstandard conditions: Pressure of CH3OH= 15.0 mmHg.
  6. chemistry

    calculate the mass carbon monoxide, CO, that was needed to produce 78g of methanol, CH3OH, by the following reaction: 2H2 + CO - CH3OH.
  7. chemistry - grade 9

    calculate the mass carbon monoxide, CO, that was needed to produce 78g of methanol, CH3OH, by the following reaction: 2H2 + CO -> CH3OH.
  8. Chemistry

    Given the equilibrium: CO + 2H2 = CH3OH H=-18.0kJ How will the concentration of CO at equilibrium be affected by the following?
  9. chemistry

    For the equilibrium system below, which of the following would result in an increase in the concentration of CO(g)?
  10. chemistry

    CH3OH(g) ----> CO(g) + 2H2 (g) (delta H =+90.7k) A) is heat absorbed or released in the course of this reaction?

More Similar Questions