Chemistry

posted by .

I have this question and I am pretty sure on what to use to solve it but I am just stuck. The reaction of 8 g of hydrogen and 28 g of carbon monoxide gave 16 g of methanol. What was the theoretical yield if the percent yield was 50%?

actual yield
________________ X 100% = percent yield
theoretical yield

Any help or explantion of the process would be greatly appreciated.

  • Chemistry -

    (Actual/theoretical)*100 = 50
    (A/T) = 50/100 = 0.50
    A = 0.5T or
    T = A/0.5 = 2A
    Theo = 2*16(from the problem) = 32 g.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Iron ore consists mainly of iron III oxide. When iron III oxide is heated with an excess of coke(carbon), iron metal and carbon monoxide are produced. Assume that even if an excess of coke is not present that the reaction proceeds …
  2. chemistry

    the fuel methanol(CH3OH) is made by the reaction of carbon monoxide and hydrogen. a) write the balanced chemical reaction b)how many grams og hydrogen are needed to produce 45.0 grams of methanol?
  3. chem 3A

    please help me with these homework problems from chemistry because the teacher did not give enough information to some of these chemistry work problems. 1) 50.0 g of aluminum is reacted with excess sulfuric acid. The chemical equation …
  4. 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 …
  5. Chemistry

    Hydrogen and methanol (CH3OH) have both been proposed as alternatives to hydrocarbon fuels. a) Write balanced chemical equations for the complete combustion of hydrogen and the complete combustion of gaseous methanol. Combustion reaction …
  6. General Chemistry

    Methanol is produced as the sole product of the combination of carbon monoxide gas and hydrogen gas. If 3.12X103 kg of methanol are actually produced, what is the precent yield if you start with 430.0 kg of hydrogen gas?
  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

    Carbon monoxide gas and hydrogen gas are mixed in a two liter flask. The reaction produces methanol gas as the only product. At equilibrium the Keq is 1.1 x 10-5. The flask initially held 6 grams of hydrogen and the equilibrium concentration …
  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