Post a New Question

Chemistry

posted by .

Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation:

CO(g)+ 2H2(g) <---> CH3OH(g) £H = -90Kj

1. State Le Chateliers principle and explain the following:
a)The effect that increasing the pressure will have on the equalibrium yield of menthanol

b) the effect of increasing the temperature will have on the equalibrium yield of menthanol

c) the effect of increasing the temperature will have on the rate of reaction

where appropriate, show clear understanding of how the Le Chatelier's principle applies



I will be happy to critique your thinking on this.

Le Chateliers principle states that If a system in a state of equilibrium is disturbed, it will undergo a change that shifts its equilibrium position in a direction that reduces the effect of the disturbance.

Therefore,
a)If you increase pressure on a gas you decrease the volume (boyles law), the reaction will shift in a direction to the side of the reaction with the fewer moles of gas in order to reduce pressure and bring the system back to equilibrium

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem.....

    Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation: CO(g)+ 2H2(g) <---> CH3OH(g) H = …
  2. Chemistry

    Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO (g) + 2H2 (g) -> CH3OH (g) An equilibrium mixture in a 2.50 L vessel is found to contain 2.62e-2 mol CH3OH, 0.170 mol CO, and …
  3. Chemistry

    Methanol (CH3OH) is used in the production of many chemicals. methanol is made by reacting carbon monoxide and hydrogen at high temperature and pressure. CO(g) + 2H2(g) ==> CH3OH(g) a) How many moles of each reactant are needed …
  4. chemistry

    calculate the mass carbon monoxide, CO, that was needed to produce 78g of methanol, CH3OH, by the following reaction: 2H2 + CO - CH3OH.
  5. 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.
  6. chem h

    Methanol (CH3OH) is used in the production of many chemicals. methanol is made by reacting carbon monoxide and hydrogen at high temperature and pressure. CO(g) + 2H2(g) ==> CH3OH(g) a) How many moles of each reactant are needed …
  7. chemistry

    b. Methanol, CH3OH, which can be used as a fuel, can be formed by the reaction between carbon monoxide and hydrogen as depicted in the following balanced equation. 2H2 + CO ¨ CH3OH Suppose 356 g of CO and 65 g of H2 are mixed and …
  8. chemistry

    Methanol (CH3OH) is used in the production of many chemicals. Methanol is made by reacting carbon monoxide and hydrogen at high temperature and pressure. CO(g) + 2 H2(g) CH3OH(g) (a) How many moles of each reactant are needed to produce …
  9. chemistry

    Methanol CH3Oh can be produced by reacting carbon monoxide and hydrogen gas in the presence of a catalyst. If 75.00 grams of carbon monoxide reacts with 106.3 grams of hydrogen, 68.40 grams of methanol are produced. What is the percent …
  10. Chemistry (Le Chatelier's Principal)

    Methanol has the formula CH3OH and can be produced by the reaction of carbon monoxide with hydrogen gas. CO + 2 H2 <--> CH3OH + heat In an attempt to maximize the yield of methanol (amount of methanol …

More Similar Questions

Post a New Question