# Question ef04f

Nov 20, 2015

$\text{9.04 g}$

#### Explanation:

From what I can tell looking at the equation given to you, you're dealing with the decomposition of glucose in the presence of sulfuric acid.

This is essentially a dehydration reaction because the glucose molecules are losing water molecules.

The balanced chemical equation for this reaction can be written like this

${\text{C"_6"H"_12"O"_text(6(s]) stackrel(color(red)("H"_2"SO"_4) color(white)(xx))(->) 6"C"_text((s]) + 6"H"_2"O}}_{\textrm{\left(l\right]}}$

Now, notice that you have a $1 : 6$ mole ratio between glucose and solid carbon. This means that the reaction will produce $6$ times more moles of carbon than you have moles of glucose taking part in the reaction.

So, how many moles of glucose do you have? Use the compound's molar mass to figure that out

22.6color(red)(cancel(color(black)("g"))) * ("1 mole C"_6"H"_12"O"_6)/(180.16color(red)(cancel(color(black)("g")))) = "0.1254 moles C"_6"H"_12"O"_6

This means that the reaction will produce

0.1254color(red)(cancel(color(black)("moles C"_6"H"_12"O"_6))) * "6 moles C"/(1color(red)(cancel(color(black)("mole C"_6"H"_12"O"_6)))) = "0.7524 moles C"

Finally, use carbon's molar mass to see how many grams would contain this many moles

0.7524color(red)(cancel(color(black)("moles C"))) * "12.011 g"/(1color(red)(cancel(color(black)("mole C")))) = color(green)("9.04 g C")#