Question

2. In the combustion of octane: 2CsHisogo 25020g 16CO. 18H2Ogn what would 2(g be the rate of formation of CO2 if the concentration of octane was changing at a rate of 0.25mol/Ls? a)Referring to the preceding question, if the rate of formation of H2O is 0.900 mol/Ls, what is the rate of reaction of CsHis? b)At what rate will o2 be reacting under the conditions in question #2? c)If octane is burning at a constant rate of 0.25mol/s, how many moles of it will burn in 15 minutes?

I'm very confused. If someone could please explain how to solve this problem I'd greatly appreciate it.

Answer 1

ANSWER:

According to the question from 2 moles of Octane, 16 moles of CO2 forming

In the question 0.25 moles of Octane given

2 ............................ 16

0.25 ..................     ?

= 0.25 x16/2

= 2

Hence the rate of formation of CO2 is 2 mol/L.

a) According go the question:

2 moles of octane ..................................   18 moles of H2O

?                        .......................................... 0.9

= 0.9 x 2 / 18

= 0.161 moles /L.

Hence the number of moles of Octane required = 0.161

b) According to the question for 2 moles of Octane 25 moles of O₂ required.

C) Combustion is the Zero order reaction it is independent on the Intial concentration of the reactant.