Orsat Analysis on Furnace burning

[nobodyuknow]

Homework Statement

Consider a continuous, steady state process to produce hydrogen in which the following reactions take place:

C6H12 + 6H2O -> 6CO + 12H2 (desired reaction)
C6H12 + H2 -> C6H14 (undesired reaction)

In the process 220 mol of C6H12 and 840 mol of H2O is fed into the reactor each hour. If the yield of H2 is 48% and the selectivity of H2 relative to C6H14 is 10.5:

Which component is the limiting reagent?

What is the % excess of the excess reagent?

Calculate the molar flow rates of all the components in the outlet fas.

Silicon (Si) is prepared for use in the semiconductor industry by reaction and separation in a two stage process as shown below.

http://prntscr.com/idts4

The solid Si is reacted with gaseous hydrogen chloride (HCl) to form several polychlorinated silanes. If 100kg of Si (solid) is reacted, what mass of trichlorosilane (HSiCl3) is produced?

Homework Equations

The Attempt at a Solution

If someone could start me off (the VERY, VERY start) as I don't understand this part of the question 'In the process 220 mol of C6H12 and 840 mol of H2O is fed into the reactor each hour. If the yield of H2 is 48% and the selectivity of H2 relative to C6H14 is 10.5:'
it would be much appreciated.

 

[nate808]

Hello!

First, let's define some terms that are mentioned in the problem:

- Yield of H2: This refers to the amount of H2 that is actually produced in the desired reaction (C6H12 + 6H2O -> 6CO + 12H2) compared to the amount that could potentially be produced if all of the reactants were converted into products. In this case, the yield is given as 48%, meaning that for every 100 moles of H2O that is fed into the reactor, only 48 moles of H2 are actually produced.

- Selectivity of H2 relative to C6H14: This refers to the ratio of H2 produced in the desired reaction (C6H12 + 6H2O -> 6CO + 12H2) compared to the amount of C6H14 produced in the undesired reaction (C6H12 + H2 -> C6H14). In this case, the selectivity is given as 10.5, meaning that for every 1 mole of C6H14 produced, 10.5 moles of H2 are produced in the desired reaction.

Now, to answer the first question - which component is the limiting reagent? To determine this, we need to look at the stoichiometry of the desired reaction. From the balanced equation, we can see that for every 1 mole of C6H12, 12 moles of H2 are produced. Therefore, in order for all of the H2 to be consumed in the reaction, we would need 12 moles of C6H12. However, we are only feeding 220 moles of C6H12 into the reactor, so this means that C6H12 is the limiting reagent.

To find the % excess of the excess reagent (in this case, H2O), we need to first calculate the amount of H2 that would be produced if all of the C6H12 was consumed in the reaction. Since we have 220 moles of C6H12 and the stoichiometry of the reaction is 1:12 for C6H12 to H2, this means that we would produce 220*12 = 2640 moles of H2. However, we know that the actual yield of H2 is only 48%, so the actual amount of H2 produced would be