a) If 4.0g of hydrogen are made to react with excess carbon monoxide, how many grams of methanol can theoretically be produced according to the equation?
b) If 28.0g of methanol are actually produced, what is the percent yield?
2007-11-11 10:12:11 · 2 answers · asked by fretdancer 1 in Science & Mathematics ➔ Chemistry
In this problem, we have all the CO we can possible use, and all the H in CH3OH comes from H2. From the equation, in 1 mole of CH3OH, 4 grams are hydrogen, so the answer is the weight of 1 mole of CH3OH. or 32.
28 grams is 7/8th of 32. The yield is then 87.5%.
2007-11-11 10:27:18 · answer #1 · answered by cattbarf 7 · 0⤊ 0⤋
confident, that's how CH3OH is formed. Now to stability the equation you place a stoichiometric coefficient of two in front of the H2. Calculate your moles for each by ability of way of dividing by ability of way of the molar mass. as straight away as you have it in moles you will see that which you circulate with 2 moles of H2 to make a million mole of CH3OH. to confirm the theoretical yield of this, you multiply the quantity of moles of H2 by ability of way of the mole ratio of H2 to CH3OH (a million:2 or .5), and this might present day you which ones contain your answer.
2016-12-08 18:56:39 · answer #2 · answered by ? 4 · 0⤊ 0⤋