18. Consider the following reaction:
CO(g) + 2H, (g) → CH,OH(g)
(a) How many moles of H, are required to react completely with 2 mol of CO?
(b) How many H, molecules would be needed to consume 2 mol of CO? How many Hatoms would be needed?
(c) How many grams of H, are required to consume 2 mol of CO?
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Answers
Answer:first calculate the number of moles available for each reactant.
No. of moles of H2= mass/relative molecular mass
= 1.20g/2
= 0.6moles
No. of moles of CO= mass/ relative molecular mass
= 7.45g/ (12+16)
= 0.2661moles.
The equation of the reaction is: CO(g)+2H2(g) --> CH3OH(l)
According to the equation,
1 mole of CO reacts with 2 moles of H2.
0.2661 mole of CO reacts with 0.5322 moles of H2. (this statement shows that H2 is in excess since 0.6moles (as calculated abv.) is available)
0.3mole of CO reacts with 0.6 moles of H2 (this statement shows that CO is limiting because there's only 0.2661 moles of CO available)
Answer: The limiting reactant is CO.
To find the theoretical yield, we always have to take into consideration the limiting reactant of the reaction which is this case, is, CO. This is so as the limiting reactant will affect the result of the reaction due to its restrictive amount available.
According to the equation,
1 mole of CO reacts with 2 moles of H2 to produce 1 mole of CH3OH.
0.2661 mole of CO reacts with 0.5322 moles of H2 to produce 0.2661 mole of CH3OH (by ratio)
As seen from the abv statement, the theoretical yield of CH3OH (in mole) is 0.2661.
Theoretical yield (in grams)= no of moles x relative molecular mass
= 0.2661 mole x (12+3+16+1)
= 0.2661 mole x 32
= 8.5152 grams
= 8.52 grams (to 3 sf)
Answer: 8.52 grams
Reactant present in excess is H2 (as shown above).
No. of moles of H2 available: 0.6 mole
No of moles of H2 used: 0.5322 mole
No of moles of H2 left over: 0.6-0.5322mole
= 0.0678mole
Mass of H2 left over: No of moles x relative molecular mass
= 0.0678mole x 2
= 0.1356 grams
= 0.136 grams (to 3sf)
Answer: 0.136g
We all know that percentage yield = (actual yield/ theoretical yield) x 100%
88% =(actual yield/ 8.52g (from q2) x 100%
Actual yield = 7.4976g
Actual yield = 7.50g (to 3 sf)
Answer:7.50g
Answer:
hope it is helpful to you.
Explanation:
c)7.50g
