Homework Help: chemistry

Posted by jenny on Wednesday, December 28, 2011 at 8:38am.

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 Би CH3OH Suppose 356 g of CO and 65 g of H2 are mixed and allowed to react.
(i)
Which species is the limiting factor in the overall reaction? Explain the reason for your answer.
(ii)
Calculate the amount of methanol that could, theoretically, be produced.
(iii)
If 352 g of methanol was actually produced, what is the percentage yield for your reaction?

chemistry - drwls, Wednesday, December 28, 2011 at 9:01am
(i) Convert the masses of reactants to moles. 356 g of CO is 356/28 = 12.7 moles. 65 g of H2 is 65/2.016 = 32.2 moles. There are MORE than twice as many moles of H2, compared to CO, so CO is the limiting reactant.
(ii) The number of moles of CH3OH that can be produced is 12.7 . That equals the number of moles of CO available. That mass of CH3OH formed is
12.7*(32.03) = 406.8 g
(iii) 352/406.8 = ___ yield
(convert to %)

Answer this Question

Related Questions

chemistry - the fuel methanol(CH3OH) is made by the reaction of carbon monoxide ...
chemistry - calculate the mass carbon monoxide, CO, that was needed to produce ...
chemistry - grade 9 - calculate the mass carbon monoxide, CO, that was needed to...
Chemistry - Methanol (CH3OH) is used in the production of many chemicals. ...
Chemistry - Methanol (CH3OH) is produced commercially by the catalyzed reaction ...
chemistry - 2. Methanol, CH3OH, is used as fuel in race cars. This liquid fuel ...
chem h - Methanol (CH3OH) is used in the production of many chemicals. methanol...
chemistry - Methanol (CH3OH) is used in the production of many chemicals. ...
chemistry - Methanol (CH3OH) is used in the production of many chemicals. ...
Chem..... - Methanol, CH3OH, is produced on an industrial scale from carbon ...

For Further Reading

First Name:
School Subject:
Answer: