Deadline: June 15th. ( School closes on that day, and I can't submit my Chemistry Study Journals for Extra Credit, afterward. ) Hi, I'm studying in a Chemistry journal, and got stuck on a practice question:
If 5 moles of carbon monoxide react with 2.3 moles of hydrogen gas, how many moles of methanol can be produced?
CO + 2H2 → CH3OH

So I was wondering if I would use a balanced equation, or like, solve it like one, or something like that. I dunno, I'm kinda lost, stuck I guess...

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Explanation:c

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Read it CAREFULLY: It's a balanced equation, so your gonna have to solve it like one.

We have 5 moles of carbon monoxide, reacting to 2.3 moles of hydrogen gas.

So the answer would be from a balanced equation.

Use a periodic element table to figure out the rest.

It should be easy from here.

I hope this helps. :D

Explanation:

From the equation:

CO + 2H2 → CH3OH

Adding 1 to CO and CH3OH

1 CO + 2 H2 → 1 CH3OH

So the ratio of CO, H2 and CH3OH is 1:2:1

That means: 1 mole of CO will react with 2 moles of H2 to form 1 moles of CH3OH

With 5 moles of CO and 2.3 moles of H2, there are more CO than H2. So H2 is the limiting factor.

Going with the 2:1 ration, there will be 2.3/2 = 1.15 moles of CH3OH produced.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.